AP Chemistry · Web view10.14 Arrange the following AFn species in order of increasing F-A-F bond angles: BeF3, BeF2, CF4, NF3, OF2. 10.16 State ideal values for each of the bond angels

AP Chemistry Mr. Brombach

Semester A

HW #11.12.42 Magnesium has naturally occurring isotopes, 24Mg, and 26Mg. what is the mass number of each isotope? How many protons, neutrons, and electrons are present in each?

2.46 Gallium has two naturally occurring isotopes, 69Ga (isotopic mass 68.9256 amu, abundance 60.11%) and 71Ga (isotopic mass 70.9247 amu, abundance 39.89%). Calculate the atomic mass of gallium.

1.27.8 A radio wave has a frequency of 3.4 × 1010 Hz. What is the energy (in J) of one photon of this radiation?

7.10 Rank the following photons in terms of increasing energy: (a) blue (λ= 660nm); (c) yellow (λ = 595 nm).

7.14 Colbalt-60 is a radioactive isotope used to treat cancer of the brain and other tissues. A gamma ray emitted by an atom of this isotope has an energy of 1.33 MeV (million electron volts; 1 eV= 1.602 × 10-19 J). What is the frequency (in Hz) and wavelength (in m) of this gamma ray?

1.37.25 Use the Rydberg equation (Equation 7.3) to calculate the wavelength (in nm) of the photon emitted when a hydrogen atom undergoes a transition from n =5 to n=2.

7.27 What is the wavelength (in nm) of the least energetic spectral line in the ultraviolet series of the H atom?

1.47.45 The yellow color of sodium flame test is due to emission of photons of wavelength 589 nm. What is the mass equivalence of one photon of this wavelength (1 J kg . m2/s2)?

1.57.50 What feature of an orbital is related to each of the following?(a) Principal quantum number (n)(b) Azimuthal quantum number (l)(c) Magnetic quantum number (m1)

7.51 How many orbitals in an atom can have each of the following designations?(a) 1s; (b) 3d; (c) 4p; (d) n=3

7.53 Give all possible m1 values for orbitals that have each of the following: (a) l=2; (b) n=1; (c) n=4, l=3.

7.57 For each of the following, give the sublevel designation, the following m1 values, and the number of possible orbitals: (a) n=4, l=2; (b) n=5, l+1, (c) n=6, l=3.

7.59 For each of the following subshells, give the n and l values and the number of possible orbitals: (a) 5s; (b) 3p; (c) 4f. (see next page)7.61 Are the following quantum number combinations allowed? If not, show two ways to correct them:(a) n=2; l=0; m1 = -1 (b) n=4; l=3; m1 =1 (c) n=3; l=1; m1 = 0 (d) n=5; l=2; m1 = +3

7.62 Are the following quantum number combinations allowed? If not, show two ways to correct them: (a) n=1; l=0; m1 = 0 (b) n=2; l=2; m1 = +1 (c) n=7; l=1; m1 = +2 (d) n=3; ; l=1; m1 = -2______________________________________________________________________________

HW # 22.18.8 How many electrons in an atom can have each of the following quantum number or sublevel designations? (a) n=2, l=1; (b) 3d; (c) 4s

8.16 write a full set of quantum numbers for the highest energy electron in the ground-state B atom.

2.2 8.18 write a set of quantum numbers for the following:(a) The outermost electron in an RB atom(b) The electron gained when an S- ion becomes an S2- ion(c) The electron lost when an Ag atom ionizes

8.28 Identify each element below by its condensed electron configuration, and give the symbols of the other elements in its group:(a) [He] 2s22p1 (b) [Ne] 3s23p4

(c) [Xe] 6s25d1 (d) [Ar] 4s23d104p4

(e) [Xe] 6s24f145d2 (f) [Ar] 4s23d5

2.38.22 Write the symbol, group number, and period number of the element represented by each of the following condensed electron configuration: (a) [He] 2s22p4; (b)

8.24 Draw an orbital diagram showing valence electrons, and write the condensed ground-state electron configuration for each of the following elements: (a) Ti; (b) Cl; (c) V; (b) Ba; (e) Co.

8.26 How many inner electrons, outer electrons, and valence electrons are present in an atom of the following elements? (a) O; (b) Sin; (c) Ca; (d) Fe; (e) Se

2.48.40 Arrange each set of atoms in order of increasing atomic size: (a) Rb, K Cs; (B) c, o, Be; (c) Cl, K, S; (d) Mg, K, Ca.

2.58.34 In what region of the periodic table will you find elements with relatively high IEs? With relatively low IEs?

8.42 Arrange each set of atoms in order of increasing IE1: (a) Sr, Ca, Ba; (b) N, B Ne; (c) Br, Rb, Se; (d) As, Sb, Sn. 8.44 Write the full electron configuration of the Period 2 element with the following successive IEs (in KJ/mol): IE1= 801; IE2 = 2427; IE3 = 3659; IE4 = 25,022; IE5 = 32,8228.46 Which element in the following sets would you expect to have the highest IE2? (a) Na, Mg, Al; (b) Na, K, Fe

2.68.37 Which group in the periodic table has elements with high IE1 and very negative first electron affinities (EA1)? What is the charge on the ions that these atoms form?

8.59 Write the charge and full ground-state electron configuration of the monatomic ion most likely to be formed by each of the following: (a) Cl; (b) Na; (c) Ca; (d) P (e) Mg; (f) Se

8.61 How many unpaired electrons are presented in the ground state of an atom from each of the following groups? (a) 2A(2); (b) 5A(15); (c) 8A(18); (d) 3A(13)______________________________________________________________________________

HW # 3 3.19.4 Which member of each of the following pairs is more metallic: (a) Na or Cs; (b) Mg or Rb; (c) As or N?

9.6 State the type of bonding-ionic, covalent, or metallic-you would expect in (a) CsF(s); N2(g); (c) K(s); (d) BrCl(g); (e) NO(g); (f) LiCl(s)

3.29.8 Draw3 Lewis electron-dot symbols for each of the following atoms: (a) Rb; (b) Ge; (c) I; (d) Ba; (e) Xe. 9.14 Use condensed electron configurations and Lewis electron-dot symbols to depict the monatomic ions formed from each of the following, and predict the compound’s formula: (a) Ba and Cl; (b) Sr and O; (c) Al and F. 9.16 What is the periodic table group of X in each of the following ionic compound formulas: (a) XF2; (b) MgX; (c) X2SO4?

9.18 For each of the following pairs, choose the compound with the higher (more) negative) lattice energy, and explain your choice: (a) BaS or CsCl; (b) LiCl or CsCl; (c) CaO or CaS.

3.39.26 For single bonds between similar types of atoms, how does the strength of the bond relate to the size of the atoms? Explain.

9.29 Using the periodic table only arrange the members of each of the following sets in order of increasing bond strength. (a) Br-Br, Cl-Cl, I-I; (b) S-H, S-Br, S-Cl; (c) C== N, C-N, C==N.

9.41 Using EN values, indicate the polarity of the following bonds with polar arrows, and determine the more polar bonds in each pair (a) N-B ORN-O; (b) C-S or S-O; (c) N-H or N-O

. 9.43 Are the bonds in each of the following substances ionic, nonpolar, covalent, or polar covalent? Arrange the substance with polar covalent bonds in order of increasing bond polarity: (a) S8; (b) RbCl; (c) PFS; (d) SCl2; (e) F2; (f) SF2. 9.45 Rank the members of each of the following sets of compounds in order of increasing ionic character of their bonds. Use polar arrows to indicate the bond polarity: (a) HBr, HCl HI; (b) H2O, CH4, HF; (c) SCl2, PCl3 SiCl4.

3.410.35 Are the following statements true or false? Correct any that is false.(a) Two σ bonds compromise a double bond. (b) A triple bond consists of one п bond and two σ bonds.(c) Bonds between atomic s orbitals are always σ bonds.(d) A п bond restricts rotation about the σ- bond axis. (e) A п bond consists of two pairs of electrons.

10.42 Describe the types of bonds and orbitals in the following: (a) NO3-; (b) CS2; (c) CH2O; (d) FNO; (e) C2F4.

HW # 4 4.19.52 Draw a Lewis structure for (a) SiF4; (b) SeCL2; (c) COF2 (C central); (d) PH4 +; (e) C2F4.

9.54 Draw Lewis structure of all the important resonance forms of each of the following: (a) NO2; (b) NO2F (N central); (c) HNO3 (HONO2).

9.56 Draw a Lewis structure in the following g: (a) IF5; (b) AlH4-; (c) COS (C central). 9.58 Draw a Lewis structure for the most important resonance from of the following, showing charges of the atoms: (a) BrO3-; (b) SO3

2-

9.60 The following species do not obey the octet rule. Draw a Lewis structure for each one state the type of octet rule exception: (a) BH3; (b) AsF4-; (c) SeCl4; (d) PF6-; (e) ClO3.

4.2.9.58 Draw a Lewis structure for the most important resonance form of the following, showing formal charges and oxidation numbers of the atoms: (a) BrO3

-; (b) SO32-

9.60 The following species do not obey the octet rule. Draw a Lewis structure for each one and state the type of octet rule exception: (a) BH3; (b) AsF4

-; (c) SeCl4; (d) PF6- (e)

ClO3-.

4.310.36 What is the hybridization of nitrogen in each of the following ions or molecules? (a) NO; (b) NO2; (c) NO2

-; (d) NO3-

10.38 For each of the following molecules, which types of atomic orbitals of the central atom mix to from hybrid orbitals? (a) SiH3Cl; (b) CS2; (c) Cl2O

4.410.7 What would you expect to be the electron-group arrangement around atom A in each of the following case? For Each arrangement, give the ideal bond angle and the direction of any expected deviation:

10.8 Determine the electron-group arrangement, molecular shape, and ideal bond angle(s) for each of the following: (a) O3; (b) H2O+; (c) NF3; (d) SO4

2-.

4.510.10 Determine the molecular shape, ideal bond angle(s), and the direction of any deviations from these angles for each of the following: (a) ClO2-; (b) PF5; (c) SeF4; (d) KrF2.

10.14 Arrange the following AFn species in order of increasing F-A-F bond angles: BeF3, BeF2, CF4, NF3, OF2.

10.16 State ideal values for each of the bond angels in the following molecules and where you expect deviations: (see textbook)4.610.23 A molecule of formula BY3 is found experimentally to be polar. Which molecular shapes are possible and which impossible for BY3?

10.25 Consider the following molecules: SCl2, F2, CS2, CF4, BrCl.(a) Which has the most polar bonds?(b) Which have a molecular dipole moment?

10.27 Which molecule in each of the following pairs has the greater dipole moment? Give the reason for your choice. (a) SO2 or SO3 (b) ICI or IF (c) SiF4 or SF4 (d) H2O or H2S

4.710.56 For the following ions, predict the shape, state the hybridization of the central atom, and give the ideal bond angles and any expected deviations: (a) BrO-; (b) AsCl4

-; (c) SeO4

2-; (d) BiF52-; (e) SbF4

+; (f) AlF63-; (g) IF4

+.

(a) X │

X― A: │ X ¨

X―A―X

HW # 55.1 11.19 What is the strongest interparticle force that occurs in sample of each of the following substances? (a) CH3OH; (b) CCL4; (c) NaL; (d) H3PO4; (e) SO2

5.211.16 Polar molécules exhibait dipole-dipole forces. Do they also exhibit dispersion forces? Explain.

11.23 Draw each of the following H-bonded structure (a) (HF) 2 dimer; (b) (CH3OH) 4 cyclic

5.311.1 How does the energy of attraction between particles compare with their energy of motion (a) in a gas; (b) in solid?

11.4(a) Why is the heat of fusion (ΔHfus) of structure smaller than its heat of vaporization (ΔHvap)?(b) Why is the heat of Sublimation (ΔHvap) of a substance greater than its ΔHvap?(c) At a given temperature and pressure, how does the magnitude of the heat of vaporization of a substance compare with its heat of condensation?

11.5 Which of the following forces are intermolecular and which intermolecular? (a) Those preventing oil from evaporating at room temperature(b) Those preventing butter from melting in a refrigerator(c) Those allowing silver to tarnish(d) Those preventing 02 and n2 in the air from reacting to form NO

5.411.105 consider the phrase diagram for substance X:(a) What phrase(s) is (are) present at point A? E? F? H? B?(b) Which point corresponds to the critical point? Which point corresponds to the triple point?(c) What curve corresponds to the conditions at which the solid and gas are in equilibrium? (d) Describe what happens when you start at point H and decrease the pressure at constant temperature.(f) is liquid X more or less dense than solid X?

11.108 The density of solid gallium at its melting point is 5.9 g/cm3, whereas that of liquid gallium is 6.1 g/cm3. Is the temperature at the triple point higher or lower than the normal melting point? Which direction is the slope of the solid-liquid curve on the gallium phase diagram?

11.57 For the metals listed, the number of atoms per unit cells is given in parentheses. What type of cubic lattice does each metal form? (a) Po (l); (b) Fe (2); (c) Ag (4)

5.511.37 Rank the following compounds in order of increasing surface tension a given temperature, and explain your ranking: (a) CH3 CH2 CH2 OH (b) HOCH2CH(OH)CH2OH (c) HOCH2CH2OH

11.39 Rank the compounds in problem 11.37 in order of increasing viscosity at given temperature, and explain your ranking.

5.611.32 Why does the antifreeze ingredient ethylene glycol (HOCH2CHOH; M=62.07 g/mol) have a boiling point of 197.6 ۫C, whereas propanol (CH3 CH2 CH2 OH; M=60.09 g/mol), a compound with a similar molar mass, has a boiling point of only 97.4 ۫C

5.711.50 Both solid Kr and solid Cu consist of individual atoms. Why do their physical properties differ so much? 11.59 of the five major types of crystalline solid, which would you expect each of the following to form, and why? (a) Sn; (b) Si; (c) Xe; (d) cholesterol (C27H45OH); (e) KCL; (f) BN

HW # 6 6.15.1 How would a sample of gas differ in its behavior from a sample of liquid in each of the following situation? (a) The sample is transferred from one container to a larger one.(b) The sample is heated in an expanded container but no change of state occurs. (c) The sample is placed in a cylinder with a piston, and an external force is applied. 1.61 carry out each of the following calculations, paying special attention to significant figures, rounding, a and units (J=joule, the SI unit of energy; mol= mole, the SI unit for amount of substance);(a) (6.626×10 -34 J∙s) (2.9979×10 8 m/s) 473×10-9m(b) (6.022×10 23 molecules/mol) (1.04 × 10 2 g) 44.01 g/mol

6.21.55 Round off each of the following numbers to one fewer significant figure, and perform the calculation: 11×154×7.9 2.1×3.1×3.9

5.15 Convert the following pressures into atmospheres:(a) At the peak of MT. Everest, the pressure is only 2.7×102mmHg. (b) A cyclist fills her bike tires to 92 psi.(c) The surface of Venus has an atmospheric pressure of 9.15 ×106 Pa.(d) At 100 ft below sea level, scuba diver experiences a pressure of 2.44 × 104torr. 5.10 If the barometer reads 748.5 torr, what is the pressure of gas in the flask in atmospheres (Figure P.10)?

5.11 If the barometer reads 768.2 mmHg, what is the pressure of the gas in the flask in kilopascals (Figure P5.11)?

6.35.28 You have 207 Ml oxygen gas at 699 mmHg and 25 ۫C.What is the mass (in g) of the sample?

5.31 Hemoglobin is the protein that transports O2 through the bloods from the lungs to the rest of the body. In doing so, each molecule of hemoglobin combines with four molecules of hemoglobin combines with 1.53 mL O2 at 37C and 743 torr, what is the molar mass of hemoglobin?

6.45.39 What is the density of Xe gas at STP?

5.41 How many moles of gaseous phosphine (PH3) occupy 0.0400 L at STP? What is the density?

6.55.26 A sample of nitrogen gas is confined in a 6.0-L container at 228 torr and 27 ۫C. How many moles of gas are present in the sample?

5.29 A 75.0-g sample of argon is confined in a 3.1-L vessel. What is the pressure (in atm) at 115 ۫C? 6.6

5.47. (see textbook)

HW # 77.11.107 Classify each of the following as a compound, a homogenous, or a heterogeneous mixture: (a) distilled water; (b) gasoline; (c) beach sand; (d) wine; (e) air. 2.109 name the technique(s) and briefly describe the procedure you would use to separate the following mixture into two components: (table salt and pepper; (b) table sugar and sand;

7.2 (see textbook)12.11 What is the strongest type of intermolecular force between solute and solvent in each of the following solutions: (a) CsCl(s) in H2O(l)(b) CH2CCH3(l) in H2O(l)(c) CH3OH(l) in CC4(l)(d) Cu(s) in Ag(s) (e) CH3Cl(g) in CH3OCH2(g)(f) CH3CH3(g) in CH3 CH2 CH2 CH2 NH2(l)

12.13 Which member of the following pairs is more solute in diethylether? Why? (a) NaCl(s) or HCl(g)(b)H2O(l) or CH3CH(l)(c) MgBr2(s) or CH3MgBr(s)Diethyleher = CH3- CH2-O-CH2-CH3

7.312.60 How would you prepare these aqueous solutions:(a) 3.00 × 102 g of 0.115 m ethylene glycol (C2H6O2)(b) 1.00 kg of 2.00 mass % HNO3 from 62.0 mass % HNO3?

12.62 a solution isopropanol (C3H7OH) is made by dissolving 0.30 mol isopropanol in 0.80 mol water. (a) What is the mole fraction of isopropanol?(b) What is the mass percent of isopropanol?

7.412.54 Calculate the majority of these aqueous solutions: (a) 42.3 g table sugar (C12H22O11) in 100.0 Ml solution

12.56 How would you prepare these aqueous solutions: (a) 355 mL of 8.74 × 10 -2 M KH2PO4 from solid KH2PO4?

7.512.58 Calculate the majority of solution containing 88.4 g glycine (NH2CH2COOH) dissolved in 1.250 kg H2O

12.61 How would you prepare these aqueous solutions: (a) 1.00 kg 0.055 m ethanol (C2HOH) from ethanol and water? (b) 475 g of 15.0 mass % HCl?

7.612.83 How many moles of solute particles are present in one liter of the following aqueous solutions:(a) 0.2 M KI; (b) 0.07 M HNO3; (c) 10-4 M K2SO4; (d) 0.07 Methanol (C2H5OH)?

12.85 rank the following aqueous solutions-(I) 0.100m NaNO3; (II) 0.200 m glucose; (III) 0.100 M CaCl2 –in order of increasing (a) osmotic pressure; (b) boiling point; (c) freezing point; (d) vapor pressure at 50 ۫c

12.87 calculate the vapor pressure of the solution of 44.0 g glycine (C3H8O3) in 500.0 g water at 25 ۫C. The vapor pressure of the water at 25 ۫C is 23.76 torr. (Assume ideal behavior) 7.712.93 What is the minimum mass of ethylene glycol (C2H6O2) that must be dissolved in 14.5 kg water to prevent the solution from freezing at -10.0 ۫F? (Assume ideal behavior) 12.91 The boiling point of ethanol (C2H5OH) IS 78.5 ۫C. What is the boiling point of solution of 3.4 g vanillin (M = 152.14 g/mol) in 50.0 g ethanol? (kb of ethanol = 1.22۫C/m.)

HW # 88.1 Complete following

No Formula of Compound Name Type of Compound 1. H2CO3

2. K2SO4

3. NH4NO3

4. Al2(CrO7)3

5. Ca(CN)2

6. NaMnO4

7. Fe(CN)2

8 Sn(ClO2)4

9. LiHCO3

10. HgCr2O7

11. lithium hydrogen carbonate12. mercury(11)dichromate13. hydrofluoric acid 14. aluminum sulfite15. tin(1V)chromate16. magnesium phoshite

8.2Complete the following: identify type of reaction, and predict the products.1. Na HCO3 + HCl →2. Fe2O3 + HNO3 →3. Fe2O + Mg →4. SO2 + O2 →5. Cl2O3 + H2O →6. Ca(OH)2 →

7. Na + H2S →8. H2 +N2 →9. Mg + P →10. Na + HCl→11. FeCl3 + NaOH→

8.31) Having nitrogen gas, hydrogen gas, and oxygen gas, obtains ammonium nitrate (write down the equation for each step).2) Given the chlorine gas, hydrogen gas, oxygen gas, and calcium metal, show the way to obtain calcium chlorite.

8.4Complete the followingNa2CO3(aq) + H3PO4(aq) →HClO4(aq) + NH4Br(aq) →Ca(OH)2(aq) + H2SO4(aq) →Cr2(SO3)3(aq) + HBrO(aq) →An assignment:1. Predict the product (check the formulas of the products) 2. Indicate the sate of matter of the product (s, 1, g or aq) 3. Indentify type of reaction as either gas formation, neutralization, or precipitation4. For all of the reaction that occurs write down the total ionic equation and the net

ionic equation.

HW # 99.13.9 Calculate each of the following quantities:(a) Mass in grams of 0.74 mol KMnO4

(b) Moles of O ATOMS IN 9.22 G Mg(NO3)2

(c) Number of O atoms in 0.037 g CuSO4 . 5H2O(d) Mass in kilograms of 2.6 × 1020 molecules of SO2

(e) Moles of Cl atoms in 0.622 g C2H4Cl2

3.11 Calculate each of the following quantities: (a) Mass in grams of 5.36 mol silver carbonate (b) Mass in grams of 2.78×1021 molecule of dinitrogen tetraoxide (c) Number of moles and formula units in 57.9g potassium chlorate (d) Number of potassium ions, chlorate ions, Cl atoms, and O atoms in (c)

9.23.31 What us the molecule formula of each compound? (a) Empirical formula CH2 (M= 42.08 g/mol)(b) Empirical formula NH2 (M=32.05 g/mol)

3.33 Determine the empirical formula of each of the following compounds from the information given:(a) 0.063 mol chlorine atoms combined with 0.22 mol oxygen atoms (b) 2.45 g silicon combined with 12.4 g chlorine

3.35. An oxide of nitrogen contains 26 mass % N(a) What is the empirical formula of the oxide?(b) If the molar mass is between 100-110 g/mol, what is the molecular formula? 9.33.61 Elemental phosphorus occurs as tetratomic molecules, P4. What mass of chlorine gas is needed for complete reaction with 351 g phosphorus in the formation of phosphorus pentachloride?

3.65 Solid iodine trichloride is prepared by reaction between solid iodine and gaseous chloride to form iodine monochloride crystals, followed by treatment with additional chloride.(a) Write a balanced equation for each step.(b) Write an overall balanced equation for the formulation of iodine trichloride.(c) How many grams of iodine are added to prepare 35.8kg of final product?

9.43.67 Calculate the maximum number of moles and mass of iodic acid (HIO3) that can form when 735 g iodine trichloride reacts with 97.7 g water.

3.69 When 0.100 mol carbon is burned in a closed vessel with 8.00 g oxygen, how many grams of carbon dioxide can from? Which reactant is in excess, and how many grams of it remain after the reaction? 3.75 What is the precent yield of a reaction in which 41.5 g tungsten (VI) oxide [WO3] reacts with excess hydrogen gas to produce metallic tungsten and 9.50 mL water (d=1.00g/mL)?

3.77 When 153 g methane (CH4) and 43.0 g chlorine gas undergo a reaction that has an 80.0% yield, what mass of chloromethane (CH3Cl) forms? Hydrogen chloride is the other product.

9.53.95 How many millimeters of 0.55 M HCl are needed to react with 3.7 g CaCO3?2HCl(aq) + CAco3(s) → CaCl2(aq) + CO2(g) + H2O(l)

5.53 How many grams of phosphorus react with 41.5 L O2 at STP to form tetraphosphuras decaoxide?P4(s) + 5O2(g)→ P4O10(s) 3.97 How many grams of solid barlium sulfur form when 25. mL of 0.160 M barium chloride reacts with 68.0 mL of 0.055 M sodium sulfate? Aqueous sodium chloride is the other product.

5.55 How many grams of phosphine (PH3) can form by the reaction of 37.5g phosphorus and 83.0 L hydrogen gas at STP?P4(s) + H2(g)→ PH3(g) [unbalanced]

HW # 1010.115.3 A reaction is carried out with water as the solvent. How would th addition of more water to the reaction vessel effect the reaction rate? Explain.

15.6 A pile of flour in your kitchen counter does not ignite with a match, but the flour dust in a mill or silo can react explosively. Explain.

15.12 For the reaction C(g) →D(g), a plot of [C] versus time is shown below. How would you determine (a) The average rate over the entire experiment (b) The reaction rate at time x (c) The initial reaction rate(d) Would the values you obtained in (a), (b), and (c) be different if you plotted [D] versus time? Explain.

*See Graph in textbook page 688*10.215.15 Express the rate of each reaction ion terms of the change in concentration of each of the reactants and products for the reactions in (a) and (b):(a) 2A(g)→B(g) + C(g)(b) D(g)→3/2E(g) + 5/2F(g)(c) For the reaction in (a), when [C] is increasing at 2 mol/L . s, how fast is [A] decreasing? (d) For the reaction in (b), when [E] is increasing at 0.25 mol/L . s, how fast is [F] increasing?

15.21 Nitrogen oxide undergoes numerous decomposition and combination reactions both in industry and the environment. One of the most thoroughly studied is the decomposition of nitrogen pentaoxide:

2N2O5(g)→4NO2(g) +O2(g)At a given instant, [N205] is decreasing at the rate of 3.15 mol/L . s. what is the rate of the reaction in terms of [NO2]?

10.315.24 By the factor does the rate change in each of the following cases (assume constant temperature)?(a) a reaction is first order with respect to reactant [A] is doubled.(b) a reaction is second order with respect to reactant B and [B] is halved.(c) a reaction is second order with respect to reactant C and [C] is tripled. 15.28 Give the individual reaction order for each substance and the overall reaction for each of the following rate laws:(a) Rate = k [BrO3-] [Br-] [H+]2

(b) R ate = k [NH4=] [NO2-] (c) Rate = k [O3] 2 [O2]

15.31 For the reaction A(g) + B(g) + C(g) → D(g) *See Data in textbook page 689*(a) what is the order with respect to each reaction?(b) write the rate law. (c) what is the value of k from trial 1?

10.415.34 In the simple decomposition reaction AB(g) →A(g) +B(g)Rate = k[AB]2 and k=0.2L/mol . s. how long will it take for [AB] to reach one-third of its initial concentration of 1.50 M?

15.35 For the reaction in Problem 15.34, what is [AB] after 10.0s?

10.515.36 In the first-order decomposition reaction, 50.0 of a compound decompose in 10.5 min.

(a) What is the rate constant of the reaction?(b) How long does it take for 75.0 of the compound to decompose?

15.37 A decomposition reaction has a rate constant of 0.0012yr-1.(a) What is the half-life of the reaction?(b) How long will it take for [reactant] to reach 12.5% of its original value?

10.615.38 The rate constant of reaction is 3.7 × 10-3 s-1 at 25 ۫C and the activation energy is 43.6 kj/mol. What is the value of k at 75 ۫C?1

15.48 During a study of ammonia production, an industrial chemist discovers that the compound decomposes to its elements N2 and H2 in a first –order process. She collects the following data: Time (s) 0 1.000 2.000[NH3] (mol/L) 4.000 3.986 3.974

(a) Use graphical methods to determine the rate constant.(b) What is the half-life of ammonia decomposition?

15.55 For the reaction ABC + D <==> AB + CD, ΔH0rxn =-50 KJ/mol and Ea (fwd) = 200

KJ/mol. Assuming the reaction occurs in one step, (a) Draw a reaction energy diagram. (b) Calculate Ea(rev).

(c) Sketch a possible transition state if A-B-C is Vshaped.

End of semester A

Semester B

HW # 11 11.116.10 In which cases are Kc and Kp equal and in which cases are they not equal?

16.21 Determine Δngas for each of the following equations:(a) 2KClO3(s) <==> 2KCl(s) + 302(g) (b) 2PbO(s) + O2(g) <==> 2PbO2(s) (c) I2(s) +3XeF2(s) <==> 2IF3(s) + 3Xe(g)

16.23 calculate Kc for the following equilibria: (a) CO(g) + Cl2(g) <==> COCl2(g); Kp = 3.9 × 10-2 at 1000 K(b) S2(g) + C(s) <==> CS2(g); Kp = 28.5 at 500 K

11.216.15 The powerful chlorinating agent sulfury1 dichloride (SO2Cl2) can be prepared by the following two-step sequence:H2S(g) + O2(g) <==> SO2(g) + H2O(g)SO2(g) + Cl2(g) <==> SO2Cl2(g)a) balance each step and write the overall balanced equationb) Show that the overall Qc equals the product6 of the Qc’s for the individual steps 16.19 balance each of the following process and write its mass-action expression, Qc:(c) H2SO3(aq) <==> H2O(l) + SO2(aq)(d) H2O(l) + SO3(g) <==> H2SO4(aq) (e) KNO3(s) <==> KNO2(s) + O2(g)

16.25 At 425 ۫C, Kp is 4.18 × 10-9 for the reaction 2HBr(g) <==> H2(g) + Br2(g)In one experiment, 0.20 atm HBr(g), 0.010 atm H2(g) and 0.010 atm Br2(g) are introduced into a reaction vessel. Is the reaction at equilibrium? If not, in which direction will it proceed?

11.316.33 In an experiment to study the formation of HI(g), H2(g) + I2(g) <==> 2HI(g)H2(g) and I2(g) were placed in sealed container at a certain temperature. At equilibrium, [H2] = 6.50 × 10-5 M, [I2]=1.06 × 10=3 M, and [HI] = 1.87 × 10-3 M. calculate Kc for the reaction of this temperature.

16.37 When 0.15 mol PH3 BL3(s) is introduced into a 3.0-L container at a certain temperature, 8.4×10-3 mol PH3 is present at equilibrium: PH3BCl3(s) <==> PH 3(g) + BCl3(g)

16.39 For the following reaction, Kp is 6.5×104 atm-1 at 308K: 2NO(g)+Cl2(g) <==> 2NOCl(g)

11.416.45 Hydrogen iodine decomposes according to the reaction2HI(g) <==> 2B(g) + C(g); Kc=2.35 × 10-8 at 100۫CA sealed 1.00-L reaction vessel initially contains 1.75 ×10-3 mol A(g), 1.25 × 10-3 mol B(g), and 6.50× 10-4 mol C(g) at 100 ۫ C. when equilibrium is reached, the concentrations of A(g) is 2.15 × 10-3 M. what are the equilibrium concentrations of B(g) and C(g)?

16.47 Phosgene (COCl2) is an extremely toxic substance that forms readily carbon monoxide and chlorine at elevated temperatures: CO(g) + Cl2(g) <==> COCl2(g) If 0.350 moles of each reactant is placed in a 0.500-L flask at 600 K, what are the concentrations of each substance at equilibrium? Kc=4.95 at this temperature. 16.50 A United Nations toxicologist studying the properties of mustard gas [S(CH2CH2Cl)2], A warfare blistering agent, prepares a mixture of 0.675 mSCl2 and 0.973 M C2 H4 and allows them to react at room temperature (20 ۫C):SCl2(g) + 2C2H4(g) <==> S(CH2CH2Cl)2 (g) At equilibrium, 0.350 M S(CH2CH2Cl)2 is present. Calculate Kp.

11.516.59 predict the effects of increasing the container volume on the amounts of reactants and products in each of the following:(a) F2(g) <==> 2F(g)(b) 2CH4(g) <==> C2H(g) + 3H2(g) (c) CH3OH(l) <==> CH3OH(g)

16.61 How would you adjust the volume of the reaction vessel to maximize product yield in the following reactions? (a) Fe3O4(s) + 4H 2(g) <==> 3Fe(s) + 4H2O(g) (b) 2C(s) + O2(g) <==> 2CO(g)

16.63 predict the effect of increasing the temperature on the amounts of products in the following reactions: (a) C O(g) + 2H2(g) <==> CH3OH(g); ΔH ۫rxn = - 90.7 kj(b) C(s) + H2O(g) <==> CO(g) + H2(g); ); ΔH۫rxn = + 131 kj (c) 2NO2(g) <==> 2NO(g) + O2(g) (endothermic) (d) 2C(s) +O2(g) <==> 2CO(g) (exothermic)

HW # 11 11.116.10 In which cases are Kc and Kp equal and in which cases are they not equal?

16.21 Determine Δngas for each of the following equations:

(a) 2KClO3(s) <==> 2KCl(s) + 302(g) (b) 2PbO(s) + O2(g) <==> 2PbO2(s) (c) I2(s) +3XeF2(s) <==> 2IF3(s) + 3Xe(g)


11.216.15 The powerful chlorinating agent sulfury1 dichloride (SO2Cl2) can be prepared by the following two-step sequence:H2S(g) + O2(g) <==> SO2(g) + H2O(g)SO2(g) + Cl2(g) <==> SO2Cl2(g)a) Balance each step and write the overall balanced equationb) Show that the overall Qc equals the product6 of the Qc’s for the individual steps 16.19 balance each of the following process and write its mass-action expression, Qc:(c) H2SO3(aq) <==> H2O(l) + SO2(aq)(d) H2O(l) + SO3(g) <==> H2SO4(aq) (e) KNO3(s) <==> KNO2(s) + O2(g)

16.25 At 425 ۫C, Kp is 4.18 × 10-9 for the reaction 2HBr(g) <==> H2(g) + Br2(g)In one experiment, 0.20 atm HBr(g), 0.010 atm H2(g) and 0.010 atm Br2(g) are introduced into a reaction vessel. Is the reaction at equilibrium? If not, in which direction will it proceed?


16.37 When 0.15 mol PH3 BL3(s) is introduced into a 3.0-L container at a certain temperature, 8.4×10-3 mol PH3 is present at equilibrium: PH3BCl3(s) <==> PH 3(g) + BCl3(g)Calculate Kc for the reaction at this temperature.

16.39 For the following reaction, Kp is 6.5×104 atm-1 at 308K:

2NO(g)+Cl2(g) <==> 2NOCl(g)

At equilibrium PNO=0.35 atm and Pcl2 = 0.10atm. What is the equilibrium partial pressure of NOCl(g)?


16.47 Phosgene (COCl2) is an extremely toxic substance that forms readily carbon monoxide and chlorine at elevated temperatures: CO(g) + Cl2(g) <==> COCl2(g) If 0.350 moles of each reactant is placed in a 0.500-L flask at 600 K, what are the concentrations of each substance at equilibrium? Kc=4.95 at this temperature. 16.50 A United Nations toxicologist studying the properties of mustard gas [S(CH2CH2Cl)2], A warfare blistering agent, prepares a mixture of 0.675 mSCl2 and 0.973 M C2 H4 and allows them to react at room temperature (20 ۫C):SCl2(g) + 2C2H4(g) <==> S(CH2CH2Cl)2 (g) At equilibrium, 0.350 M S(CH2CH2Cl)2 is present. Calculate Kp.




HW # 11 11.116.10 In which cases are Kc and Kp equal and in which cases are they not equal? 16.21 Determine Δngas for each of the following equations:(a) 2KClO3(s) <==> 2KCl(s) + 302(g) (b) 2PbO(s) + O2(g) <==> 2PbO2(s) (c) I2(s) +3XeF2(s) <==> 2IF3(s) + 3Xe(g)


11.216.15 The powerful chlorinating agent sulfury1 dichloride (SO2Cl2) can be prepared by the following two-step sequence:H2S(g) + O2(g) <==> SO2(g) + H2O(g)SO2(g) + Cl2(g) <==> SO2Cl2(g)

16.19 balance each of the following process and write its mass-action expression, Qc:(c) H2SO3(aq) <==> H2O(l) + SO2(aq)(d) H2O(l) + SO3(g) <==> H2SO4(aq) (e) KNO3(s) <==> KNO2(s) + O2(g)

16.25 At 425 ۫C, Kp is 4.18 × 10-9 for the reaction 2NOBr(g) <==> 2NO(g) + Br2(g)In one experiment, 0.20 atm HBr(g), 0.010 atm H2(g) and 0.010 atm Br2(g) are introduced into a reaction vessel. Is the reaction at equilibrium? If not, in which direction will it proceed?


16.37 When 0.15 mol PH3 BL3(s) is introduced into a 3.0-L container at a certain temperature, 8.4×10-3 mol PH3 is present at equilibrium: PH3BCl3(s) <==> PH 3(g) + BCl3(g)

16.39 For the following reaction, Kp is 6.5×104 atm-1 at 308K: 2NO(g)+Cl2(g) <==> 2NOCl(g)


16.47 Phosgene (COCl2) is an extremely toxic substance that forms readily carbon monoxide and chlorine at elevated temperatures: CO(g) + Cl2(g) <==> COCl2(g) If 0.350 moles of each reactant is placed in a 0.500-L flask at 600 K, what are the concentrations of each substance at equilibrium? Kc=4.95 at this temperature.

16.50 A United Nations toxicologist studying the properties of mustard gas [S(CH2CH2Cl)2], A warfare blistering agent, prepares a mixture of 0.675 mSCl2 and 0.973 M C2 H4 and allows them to react at room temperature (20 ۫C):SCl2(g) + 2C2H4(g) <==> S(CH2CH2Cl)2 (g) At equilibrium, 0.350 M S(CH2CH2Cl)2 is present. Calculate Kp.




HW # 1212.1 17.32give the formula of the conjugate acid of the following acids: (a) HCl (b) H2CO3 (c) H2O (d) HPO4

2- (e )NH4+ (f) H2O 17.34 in the following equations label the acids, the basis, and the conjugate acid-base pairs: (a) HCl + H2O <==> Vl- + H2O+ (b) HCIO4 + H2SO <==> ClO4-+H3SO+(c) HPO4

2 - + HSO4 <==> H2PO4- + SO42-

(d) NH4 + CN- <==> NH3 + HCN (e) H=O +HS- <==> OH- + H2S 12.217.9 use table 17.2 to rank the following in order of increasing acid strength: HIO3, HI, CH3COOH, HF.

17.11 Classify eacj of the following as a strong or weak acid or base: (a) H3AsO4 (b) Sr(oh)2 (c) HIO (d) HCIO4 (e) CH3NH2 (f) K2O

17.99 Which of the following are Lewis acids and which are Lewis bases?(a) Be2+ (b) Cl- (c) SnCl2 (d) F2O (e) Na+ (f) NH3 17.101 identify the Lewis acid and the Lewis base in each of the following equations: (a) Na+ + 6H2O <==> Na (H2O)6

+

(b) CO2 + H2O <==> H2CO3

(c) F- + BF3 <==> BF4

12.317.17 (a) What is the pH of 0.0111 M NaOH? Is the solution neutral, acidic, or basic? (b) What is the pOH of 1.23×10-3 M HCl? Is the solution neutral, acidic, or basic?

17.19 (a) What are the [H3O+], [OH-], and pOH in a solution with pH 9.78?(b) What are the [H3O+], [OH-], and pOH in a solution with pOH 10.43?

12.417.44 A 0.15 M solution of botanic acid, CH3CH2CH2COOH, contains 1.51 × 10-3 M H3O+. What is Ka for botanic acid?

17.46 Nitrous acid, HNO2, has a Ka of 7.1 × 10-4. What are [H3O+], [NO2-], in 0.50 M

HNO2?

17.48 Chloroactic acid, ClCH2 COOH, has a pKa of 2.87 what are [H3O+], p H, [ClCH2COO-1], and [ClCH2COOH] in. 1.05 M ClCH2COOH?

12.517.66 What is the p H of 0.050 M dimethylamine, (CH3)2NH?

17.68 (a) What is Kb of the acetate ion, CH3 COO-? (b) What is Ka of the anilinium ion, C6H5NH3

+?

12.617.56 Use the table 17.5 to calculate [H2S], [HS-], [S2-1], [H3O+], p H, [OH-], and pOH in a 0.10 M solution of the diprotic acid hydrosulfuric acid.

17.59 vinegar is a 5% (w/v) solution of acetic acid in a water. For culinary use, it is flavored with apples, herbs, wine, and so forth. What is the p H of vinegar?

HW # 1313.117.84 Why is a solution of NaF basic, whereas an NaCl solution is neutral?

17.86 explain with equation and, when necessary, calculations whether an aqueous solution of each of the following salts is acidic, basic, or neutral: (a) KBr (b) NH4I (c) KCN (d) Cr(NO3)2 (e) NaHS (f) Zn(CH3COO)2

13.213.2 What is the p H of 0.75 M solution of CH3NH3Cl ?

13.318.41 use Figure 18.4 to choose an indicator for the following titrations: (a) 0.10 M HCl with 0.10 M NaOH(b) 0.10 M HCOOH (table 17.2) with 0.10 M NaOH(c) 0.10 M CH3NH (table 17.6) with 0.10 M HCl

13.418.11 What are the [H3O+] and the p H of a propionate buffer that consists of 0.25 M CH3CH2COONa and 0.15 M CH3CH2COOH? Ka of paranoiac acid = 1.3 × 10-5.

18.15 What is the p H of a buffer that consists of 0.20 M NH3 and 0.10 M NH4Cl? Pkb of NH3 = 4.75

18.17 a buffer consist of 0.25 M KHCO3 and 0.32 M K2CO3. Carbonic acid is a diprotic acid with Ka1=4.5 × 10-7 and Ka2 =4.7×10-11 (a) Which Ka value is more important to this buffer?(b) What is the buffer pH?

13.518.21 A solution that contains 0.2000 M of acid, HA, and 0.1500 M of its conjugate base, A- has a ph of 3.35. What is the ph after 0.0015 mol NaOH is added to 0.5000 L of this solution?

18.23 A buffer is prepared by mixing 184 mL of 0.442 M HCL and 0.500 L of 0.400 M sodium acetate. See table 17.2 (a) What is the ph?(b) How many grams of KOH must be added to 25.0 mL of the buffer to change the ph by 0.07 units?

13.6 18.54 write the ion-product expressions for (a) Silver carbonate, Ag2CO3

(b) Barium fluoride. BaF2

(c) Copper(II) sulfide, CuS18.56 The solubility of silver carbonate is 0.032 M at 20 ۫C. Calculate the Ksp of silver carbonate.

18.58 The solubility of silver dichromate at 15 ۫C is 8.3×10-3 g/100 mL solution. Calculate the Ksp of silver dichromate.

13.718.60 calculate the molar solubility of SrCO3 (Ksp= 5.4 ×10-10) in (a) pure water and (b) 0.13 M Sr(NO3)2.

18.52 calculate the molar solubility of Ca (IO3)2 in (a) 0.060 M Ca (NO3)2 and (b) 0.060 M NaIO3. (See table 18.2)

HW # 1414.14.79 Sulfuric acid functions as an organizing agent in (a) and as an acid in (b). How do you differentiate between these two functions? (a) 4H+(aq) + SO4

2- (aq) + 2NaI(s) → 2N+(aq) + I2(s) + SO2(g) +2H2O(l)(b) BaF2(s) + 2H+ (aq) + SO4

2-(aq) → 2HF(aq) + BaSO4(s) 4.81 give the oxidation number of carbon each of the following: reaction, and explain your answer: 8NH3(g) + 6NO2(g) → 7N2(g) + 12H2O(l)

4.83 give the oxidation number of phosphorus in each of the following: (a) PH3; (b) H3PO2; (c) H3PO4; (d) H2P2O7

2-; (e) PH4+.

14.24.89 use the oxidation number method to balance the following reactions by placing coefficients in the blanks. Identify the reducing and oxidizing agents: (a) _HNO3(aq) + _K2CrO4(aq) + _Fe(NO3)2(aq)→ _KNO3(aq) +_Fe(NO3)3(aq) +_Cr(NO3)3(aq) + _H2O(l) (b) _HNO3(aq) +C2H6O(l) + _K2Cr2O7(aq) → _KNO3(aq) + _C2H4O(l) + _H2O(l) + _Cr(NO3)3(aq) (c) HCl(aq) + NH4Cl (aq) + _N2(g) +_H2O(l) (d) _KClO3(aq) + _HBr(aq) → _Br2(l) + _H2O(l) + _KCl(aq) 4.101 use the oxidation number method to balance the following reactions by placing coefficients in the blanks. Identify the reducing and oxidizing agents: (a) _CrO4

2- (aq) + _HSnO2-(aq)+ -H2O(l)→ _CrO2-(aq) + _HSnO3-(aq) + _OH-(aq)(b) _KMnO4(aq)+_NaNO2(aq) +_H2O(l)→_MnO2(s) + _NaNO3(aq) + _KOH(aq) (c) _I-(aq) + _O2(g) +_H2O(l) → _I2(s)+_OH-(aq)

14.320.25 Consider the following voltaic cell: *look on page 926 for picture* (a) In which direction do electrons flow when the switch is closed?(b) In which half-cell does oxidation occur?(c) In which half-cell do electrons enter the cell?(d) At which electrode are electrons consumed?(e) Which electrode is negatively charged?(f) Which electrode will decrease in mass during operation of the cell?(g) Suggest a solution for the cathode electrolyte.(h) Suggest a pair of ions for the salt bridge.(i) For which electrode could you use an inactive material?

(j) In which direction do cautions within the salt bridge move to maintain charge neutrality?(l) Write balanced half-reactions and an overall cell reaction. 20.27 A voltaic cell is constructed with and Sn electrode and Sn2 + electrolyte in one compartment and a Zn electrode and Zn2+ electrolyte in other compartment. Measurement shows the zinc electrode is negative. (a) Write balanced half-reactions and the overall spontaneous reaction. (b) Diagram the cell, labeling electrodes with their charges and showing the directions of electrons and cation and anion flow.

20.29 write the cell notation for the voltaic cells that incorporate each of the following redox reactions: (a) Al(s) +Cr3+(aq) → Cr(s) + Al3+(aq) (b) Cu2+(aq) + SO2(g) + 2H2O(l)→ Cu(s)+SO4

2-(aq)+4H+(aq)

14.420.33 use the emf series (Table 20.2) to arrange the following species(a) In order of decreasing strength as oxidizing agents: Fe3+, Br2, Cu2+ (b) In order of increasing strength as oxidizing agents: Ca2+, Cr2O7

2-, Ag+

20.35 balance the skeleton reactions, calculate E0 cell, and state weather or not the reaction is spontaneous(a) Co(s) +H+(aq) → Co2+(aq) + H2(g) (b) Mn2+(aq)+ Br2(l) → MnO4

-(aq)+Br-(aq) (c) Hg2

2+(aq)→Hg2+(aq)+ Hg(l)(d) Cl2(g) + Fe2+(aq) → Cl- (aq) +Fe3+(aq)

14.521.8 write balanced nuclear equations for the following:(a) Alpha decay of 234 92U (b) Electron capture by neptunium-232 (c) Positron emission by 12

7N (d) Beta decay of sodium-26

21.10 write the balanced nuclear equations for the following: (a) Formation of 48

22 Ti through position emission(b) Formation of silver -107 through electron capture (c) Formation of polonium -206 through a decay (d) Production of 241

95Am through B decay 21.12 Which nuclei would you predict to be stable: (a) 20

8O; (b) 5927 Co; (c) 9

3Li; (d) 14660Nd? Why?

14.621.38 The approximate date of an earthquake date of an earth in the San Francisco area is to be determined by measuring the 14C activity (t1/2 = 5730 yr) of parts of a tree that was uprooted during the event. The tree parts have an activity of 12.9 d/min ∙ g C, and a living tree has 15.3 d/min ∙ g C. What was the date of the earthquake?

21.81 The reaction that will probably power the first commercial fusion reactors is 31H + 2

1H → 42He + 1

0n. How much energy would be produced per mole of reaction? (Masses of atoms: 3H =3.0165 amu; 2H = 2.0140 amu; 4He = 4.00260 am

HW #15

15.16.16 If an athlete expends 1700 KJ/h playing tennis, how long would she have to play to work off 1.0 lb of body fat? (See problem 6.15) 6.21 classify the following processes as exothermic or endothermic: (a) freezing of water; (b) boiling of water; (c) digestion of food; (d) a person running; (e) a person growing; (f) wood being chopped; (g) heating with a furnace.

15.26.35 Draw an enthalpy diagram for general endothermic reaction. Label axis, reactants, products, and ΔH with its sign. 6.37 A 195-g aluminum engine part at an initial temperature of 3.00 ۫C absorbs 40.0 kj of heat. What is the final temperature of the part? (C of Al= 0.900 J/g ∙ K)

6.39 Two iron bolts of equal mass-one at 100 ۫C, the other at 55 ۫C –are placed in an insulted container. Assuming the heat capacity of the container is negligible, what is the final temperature inside the container? (C of ion=0.450 J/g ∙ K)

15.3 6.75 calculate ΔH ۫ rxn for each of the following: (a) 2H2S(g) + 3O2(g)→ 2SO2(g) + 2H2O(g)(b) CH4(g) + Cl2(g) → CCl4(l) + HCl(g) [unbalanced]

6.77 Copper(I) oxide is oxidized to copper (II) oxide according to the following equation:

Cu2O(s) + ½ O2(g) → 2CuO(s) ΔH0rxn = -146.0 KJ

Given that ΔH0f of Cu2O(s) = -168.6 KJ/mol, what is ΔH0

f of CuO(s)?

6.81 The common lead-acid car battery products large bust of current, even at low temperature, and is rechargeable. The reaction that occurs while recharging a “dead” battery is 2PbSO4(s) + 2H2O(l) → Pb(s) + 2H2SO4(l)

(a) Use ΔH0f values from appendix B to calculate ΔH0rxn.

15.5 6.53 When 1 mol NO (g) forms from its elements, 90.29 KJ of heat is absorbed. (a) Write a balanced thermochemical equation for this reaction.(b) How much heat is involved when 1.50 g NO is decomposed to its elements

6.77 copper (I) oxide is oxidized to copper (II) oxide according to the following equation:Cu2O(s) + ½ O2(g) → 2CuO(s) ΔH ۫rxn = -146.0 KJGiven that Δ H0

f of Cu20(s) = - 168.6 KJ/mol, what is ΔH0f of CuO(s)?

15.56.66 At a specific set of conditions, 341.8 KJ is given off when 1 MOL H2O(g) form sits elements. Under the same conditions, 285.8 KJ is given off when 1 mol H2O(l) forms from its elements. Calculate the heat of vaporization of water at these conditions.

6.68 Phosphorus tetrachloride is used in the industrial preparation of many organic phosphorus compounds. Equation I shows its preparation from PCl3 and Cl2: (I) PCl3(l) + Cl2(g) → PCl5(s) Use equations II and III to calculate ΔH rxn of equation I: (II) P4(s) + 6CL2(g) → 4PCl3(l) ΔH = -1280 KJ (III) P4(s) +10Cl2(g) → 4PCl5(s) ΔH= - 1774 KJ

15.619.19 predict the sign of ΔS for the following processes: (a) C2HOH(g) at 350 K and 500 torr → C2H5OH(g) at 350 K and 250 torr (b) N2(g) at 298 K and 1 atm → N2(aq)at 298 K and 1 atm (c) O2(aq) at 303 K and 1 atm → O2(g) at 303 K and 1 atm 19.21 predict which substance in each pair has the greater molar entropy and explain your choice: (a) Butane, CH3CH2CH2CH3(g) or 2-butene, (b) Ne(g) or Xe(g) (c) CH4(g) or CCl4(l) (d) NO2(g) or N2O4(g)

19.23 Without consulting Appendix B, arrange each of the following groups in order of increasing standard molar entropy, S0, and explain your choice: (a) Graphite, diamond, charcoal(b) Ice, water vapor, liquid water(c) O2,O3,O atoms (d) Glucose (C6H12O6), sucrose (C12H22O11), ribose (C5H10O5)(e) CaCO3, Ca +C + 3/2 O2, CaO + CO2

(f) SF6(g), SF4(g), S2F10(g)

15.719.42 for the oxidation of carbon monoxide to carbon dioxide,CO(g) + ½ O2(g) → CO2(g).(a) Predict the signs of ΔS ۫ and ΔH ۫ explain(b) Calculate ΔG ۫ by two different methods. 19.44 For the gaseous reaction of xenon and fluorine to from the hexafluoride (a) Calculate ΔS ۫298 = -280 (ΔH۫ 298 = -402 KJ/mol and ΔG ۫298 = -206 Kj/mol). (b) Assuming ΔS0 and ΔH0 change little with temperature, calculate ΔG ۫ at 450 K.

HW # 16

16.114.14 draw all possible skeletons for a 7-C compound with (a) 1 double bond and 6-carbon chain (b) 1 double bond and a 5-carbon chain(c) A 5-membered ring and no double bonds

14.16 add the correct number of hydrogen’s to each of the skeletons in problem 14.14

14.24 Each of the following compounds can exhibit optical activity. Circle the chiral center(s) in each: *see page 638*

16.214.20 draw the structure or give the name of the following: (a) 2, 3-imethyloctane (b) 1-ethyl-3-methylcyclohexane (c) see page 637 (d) see page 637

14.22 each of the following names are wrong. Draw structures based on them and correct the names:(a) 4-methylhexane (b) 2-ethylpentane(c) 2-methylcyclohexane (d) 3, 3-methyl-4-ethyloctane

14.24 each of the following compounds can exhibit optical activity. Circle the chiral center(s) in each: (a) see page 638 (b) see page 638

14.26 draw structures from the following names:(a) 3-bromohexane (b) 3-chloro-3-methylpentane(c) 1, 2-dibromo-2-methylbutane 14.64 in each of the following, name the functional groups (a) see page 640 (b) see page 640(c) see page 640(d) see page 640

16.414.42 determine each of the following reaction types:(a) see page 638

(b) see page 638 14.44 write equations for the following:(a) An addition reaction between H2O and 3-hexene (H+ is a catalyst) (b) An elimination reaction between 2-bromopropane and hot CH3-CH2-OK(c) A light –induced substitution reaction between Cl2 and there ethane to form 1,1 –dichloromethane

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AP Chemistry · Web view10.14 Arrange the following AFn species in order of increasing F-A-F bond angles: BeF3, BeF2, CF4, NF3, OF2. 10.16 State ideal values for each of the bond angels