2) l if λ - Teaching Center » University of Florida Final Exam Review Fall 2015 4) A compound (X) contains 49.48 % carbon, 5.191 % hydrogen, 28.87 % nitrogen, and 16.48 % oxygen

CHM2045 Final Exam Review Fall 2015

1) How many atoms of oxygen are in 35.7 g of anhydrous Copper(II) sulfate?

(1) 1.35 x 1023

(2) 5.39 x 1023

(3) 3.85 x 1023

(4) 4.04 x 1023

(5) 2.15 x 1023

2) The electronic transitions responsible for the Balmer lines in the H atom terminate

on n = 2. What is the n value for the upper level if λemitted = 410 nm?

Hint: emitted means you went down energy levels.

(1) n = 7 (2) n = 2 (3) n = 1 (4) n = 3 (5) n = 6

3) Based on ideal behavior, if a 5.0 L gas-filled balloon originally at 25°C and 2.00 atm

is changed to conditions of 1.12 atm and 15°C, what is the resulting volume of the

balloon?

(1) 2.8 L (2) 7.1 L (3) 8.6 L (4) 8.8 L (5) 9.0 L


4) A compound (X) contains 49.48 % carbon, 5.191 % hydrogen, 28.87 % nitrogen,

and 16.48 % oxygen by mass. Additionally, X’s molecular weight lies between the

domain of Compound Y’s MW and Compound Z’s MW. If MWY = 188 g/mol and

MWZ = 200 g/mol. Determine the molecular formula of the compound.

(1) C4H5N2O (2) C8H10N4O2 (3) C8H8N3O3 (4) C10H7N5O2 (5) C8H10N2O

5) Which of the following shows the correct respective valence configurations for

Fe and Cl?

(1) Fe: 4s23d8, Cl: 3p5

(2) Fe: 3d54s2, Cl: 3s23p5

(3) Fe: 4s23d6, Cl: 4d10

(4) Fe: 3d34s2, Cl: 3s23p5

(5) Fe: 3d64s2, Cl: 3s23p5

6) Which following sequence is correctly listed in order of increasing boiling point?

(1) HF < F2 < Ar < SO2

(2) SO2 < HF < Ar < F2

(3) F2 < Ar < SO2 < HF

(4) F2 < Ar < HF < SO2

(5) SO2 < Ar < F2 < HF


7) Both Mg3N2 (100.9 g/mol) and Mg(OH)2 (58.3 g/mol) can be converted to MgO (40.3

g/mol) by appropriate means. If a 2.00 g mixture of these two compounds is

converted, and 1.50 g of MgO is obtained, what is the approximate mass percent of

Mg3N2 in the mixture?

(1) 11.5% (2) 20% (3) 50% (4) 10% (5) 96%

8) If 1.86 g MgO dissolves on reaction with 100.0 mL of 1.00 M HCl (density 1.00

g/mL) in a coffee cup calorimeter, the temperature of the resulting solution

increases from 21.3 °C to 35.7 °C. Calculate the enthalpy change for the reaction per

mole of MgO dissolved. Assume that the specific heat capacity of the solution is 4.18

J/g·K and that the calorimeter has a negligible heat capacity.

(1) −6.13 kJ (2) −28.3 kJ (3) –133 kJ (4) –329 kJ (5) -613 kJ


9) Which of the following molecules is not necessarily polar?

(1) CF2I2 (2) Br2XeI2 (3) NH3 (4) CH3F (5) SO2

10) If a sheet of aluminum foil (d = 2.70 g/cm3) weighs 5.31 lbs and is 0.0130 mm thick,

the surface area of the foil is closest to…?

(1) 9.40 ft2 (2) 13.9 ft2 (3) 234 ft2 (4) 740 ft2 (5) 825 ft2


11) Element X has the valence electron configuration: ns2np4. Element M has the

valence electron configuration: ns2. Element N has the valence configuration: ns1.

What ionic compound most likely results from the reaction between M and X and N

and X?

(1) MX, N2X (2) M2X, NX (3) MX2, NX2 (4) M2X3, N2X3 (5) M3X4, N3X4

12) How many sigma (σ) and pi (π) bonds are found in CH3CH2CH2CHCHCH2COOH?

(1) 22 σ and 1 π (2) 20 σ and 2 π (3) 20σ and 3 π (4) 14 σ and 2 π (5) 20 σ and 1 π

13) If 1.951 g BaCl2·xH2O yields 1.864 g of anhydrous BaSO4 (233.43 g/mol) after

treatment with excess sulfuric acid, what is the value of x in the formula of

BaCl2·xH2O? (round to nearest whole number)

(1) one (2) two (3) three (4) four (5) five


14) Which of the following correctly distinguishes between the strengths of Li and Rb as

reducing agents?

(1) Li and Rb are equally strong reducing agents

(2) Li is a stronger reducing agent, because it more readily loses electrons

(3) Rb is a stronger reducing agent, because it more readily loses electrons

(4) Rb is a stronger reducing agent, because it more readily gains electrons

(5) Li is a stronger reducing agent, because it more readily gains electrons

15) In molecular orbital treatment of diatomic molecules, what type of molecular

orbital(s) are created by mixing an s orbital from one atom with a p orbital from the

other atom?

(1) only σ (2) only π (3) σ and π (4) σ and σ* (5) π and π*

16) If 4.00 g of element G reacts with 7.00 g of element M to produce 13.00 g of a

compound with the formula G3M4, and the atomic mass of M is 160.0 amu, what is

the atomic mass of G?

(1) 60.5 amu (2) 122.0 amu (3) 72.0 amu (4) 89.5 amu (5) 150 amu


17) Arrange the following in order of increasing size: Al3+, F−, Na+, S2−

(1) Na+ < Al 3+ < F− < S2−

(2) Al 3+ < Na+ < F− < S2−

(3) Al 3+ < F− < S2− < Na+

(4) Na+ < Al 3+ < S2− < F−

(5) Al 3+ < Na+ < S2− < F−

18) Consider the gas-phase reaction: 2 A(g) + 3 B(g) → A2B3(g). If, in an evacuated flask, a reaction occurs in a mixture of 0.5 atm of A with 1.0 atm of

B, what is the final pressure in the flask if the occurring reaction goes to completion?

(1) 0.50 atm (2) 0.96 atm (3) 1.2 atm (4) 1.7 atm (5) 4.4 atm


19) What products result from the reaction of HOSO3− acting as a Bronsted-Lowry acid

and water (OH2) acting as a Bronsted-Lowry base?

Hint: the products are the conjugate base and acid of the reaction.

Hint: Write out reaction

Hint: Write out lewis structure for (HO)2SO2 and HOSO3−. These are the true structural

forms for a common strong acid and its conjugate.

(1) (HO)2SO2, OH−

(2) SO32−, OH−

(3) (HO)2SO2, H3O+

(4) SO42−, H3O+

(5) None of these

20) Which of the following statements is correct?

(1) In an endothermic process, heat is transferred from the system to the surroundings.

(2) The greater the heat capacity of an object, the more thermal energy it produces.

(3) The SI unit of specific heat capacity is joules per gram per Celsius.

(4) Specific heat capacity has a positive value for liquids and a negative value for gases.

(5) An exothermic reaction has an enthalpy value which is negative.

(6) An endothermic reaction means you produce energy since enthalpy is positive


21) What respective type of hybridization is shown by the central atoms in CHF3 and

XeF3+?

(1) sp2, sp2 (2) sp3, sp3 (3) sp2, sp3d (4) sp3, sp3d (5) sp3, sp3d2

22) You are given solutions of HCl and NaOH and must determine their concentrations. It

takes 30.0 mL of NaOH solution to titrate 50.0 mL of 0.0782 M H2SO4. It takes 37.8 mL of

NaOH solution to titrate 100.0 mL of HCl solution. What are the concentrations of the HCl

and NaOH solutions, respectively?

(1) 0.0246 M HCl, 0.0652 M NaOH

(2) 0.344 M HCl, 0.130 M NaOH

(3) 0.0491 M HCl, 0.130 M NaOH

(4) 0.690 M HCl, 0.261 M NaOH

(5) 0.0985 M HCl, 0.261 M NaOH


23) Which hydrogen atom electron transition is associated with absorption of shortest

wavelength light?

(1) n = 3 to n = 1 (2) n = 2 to n = 3 (3) n = 3 to n = 5 (4) n = 4 to n = 1 (5) n = 1 to n = 3

24) A pure liquid with ΔH°vap = 48.5 kJ/mol exhibits a vapor pressure of 60.0 Torr at

25.0°C. Based on these data, what is the normal boiling point of the liquid?

(1) 56°C (2) 69°C (3) 75°C (4) 83°C (5) 92°C

25) Which pair of aqueous solutions is given in order of increasing freezing point?

(1) 0.010m Na3PO4 < 0.030m NaCl

(2) 0.020m NaI < 0.030m glucose

(3) 0.010m CaCl2 < 0.020m KCl

(4) 0.010m Na3PO4 < 0.020m Na3PO4

(5) 0.020m glucose < 0.010m CaCl2


26) Using the above table, determine the rate law.

(1) rate = k [A]2[B] [C]

(2) rate = k [A] [B]2[C]

(3) rate = k [A] [B][C] 2

(4) rate = k [A]2 [B]2[C]

(5) rate = k [A] [B]2[C]2

27) Using the table, determine the rate constant (L3mol-3s-1).

(1) 2.0 (2) 3.0 (3) 4.0 (4) 8.0 (5) 16.0

28) In the above table, determine the missing number.

(1) 0.025 (2) 0.040 (3) 0.400 (4) 0.029 (5) 0.016


29) Predict which solvent will dissolve more of the given solute:

left= NaCl in HCl or H2O middle= CCl4 in CHCl3 or H2O right= CH3OH in H2O or C6H14

(1) H2O, CHCl3, H2O

(2) HCl, H2O, C6H14

(3) H2O, H2O, H2O

(4) HCl, CHCl3, H2O

(5) HCl, CHCl3, C6H14

30. Consider the overall reaction: 2A + B 2C and the following mechanism

i) A + B ⇌ M (fast) ii) M+ A ⇌ 2C (slow , r.d.s.)

What would be the observed rate law for the reaction?

(1) rate = k [A] [B]2

(2) rate = k [A]2 [B] [C]

(3) rate = k [A] [B]

(4) rate = k [A]2 [B]

(5) rate = k [A] [B] [C]2


31. The decomposition of hydrogen iodide, 2HI(g) H2(g) + I2(g),

has rate constants of 9.51x10-9 L/mol-s at 500. K and 1.10x10-5 L/mol-s at 600. K.

What is the activation energy of the reaction?

(1) 1.74x103 J

(2) 1.76x105 J

(3) 1.95x10-2 J

(4) 5.38x104 J

(5) 2.12x104 J

32. Which of the following is false?

(1) Increasing the temperature increases the rate of a reaction

(2) Increasing the temperature increases the rate constant of a reaction

(3) The activation energy is the energy difference between reactants and products

(4) The activation energies of the forward and reverse reactions are different for an

exothermic reaction

(5) Lowering the activation energy increases the rate of a reaction.

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2) l if λ - Teaching Center » University of Florida Final Exam Review Fall 2015 4) A compound (X) contains 49.48 % carbon, 5.191 % hydrogen, 28.87 % nitrogen, and 16.48 % oxygen