Properties of Acids and Bases (19.1)

Collision Theory Reaction Rates1Collision Theory1) Atoms, ions, and molecules must collide in order to react.HHII

No Reaction

2Collision Theory2) Reacting substances must collide with the correct orientation.HHII

No Reaction

3Collision Theory3) Reacting substances must collide with enough energy to form the activated complex.

No ReactionHHII

4Collision Theory3) Reacting substances must collide with enough energy to form the activated complex.

HHII

HIHI5Collision Theory1) Atoms, ions, and molecules must collide in order to react.2) Reacting substances must collide with the correct orientation.3) Reacting substances must collide with enough energy to form the activated complex.

6Activated ComplexA temporary, unstable arrangement of atoms that may form products or reactants.

7Activation Energy (Ea)Minimum amount of energy needed in a collision to form the activated complex.

8Expressing Reaction RatesSome chemical reactions are very fast and others are very slow.To express the rate in clearer terms:9Calculating Reaction RatesUse the table to determine the formation rate of NO(g):CO(g) + NO2(g) CO2(g) + NO(g)[NO] @ 0.0s[NO] @ 2.0s0.000 M NO0.010 M NO[NO] @ t2 [NO] @ t1

t2 t1rate =0.005 mol/Ls0.005 mol/L*s10Reaction Rates ExampleUsing the data table, calculate the average reaction rate over the time period expressed as moles of C4H9Cl consumed per liter per second.Molarity of C4H9Cl0.00s4.00s0.220M0.100M11Comparing Reaction RatesUsing stoichiometry, we can compare the rates of two species in a reaction.C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g)If C3H8 is decreasing at a rate of 2.00 M/s, at what rate is CO2 being produced?-2.00 mol C3H83 mol CO26.00 mol CO2Ls-1 mol C3H8Ls12Discussion Questions1) What criteria must be met for reactant collisions to result in a successful product?The reactants must collide with each otherThe reactants must collide with enough energy and be in the right positionsThe reactants must have enough energy to form the activated complexB13Discussion Questions2) The most common way of expressing a reaction rate is in terms of:mol/Lg/Lsmol/Lsmol/sC14Discussion Questions3) What is the average rate of formation of salt in the first 10 seconds of this reaction?HCl + NaOH H2O + NaCl0.00 M NaCl at 0.00 s2.87 M NaCl at 10.00 s0.287 mol/L*s15Discussion Questions4) What is the average rate of formation of CO2 between 3.00 and 7.00 seconds of this reaction?H2CO3 H2O + CO21.08 M CO2 at 3.00 s3.42 M CO2 at 7.00 s0.585 mol/L*s16Discussion Questions5) Use the table to determine the average rate of sulfuric acid being consumed in this reaction between 4 and 8 seconds.2Fe + 3H2SO4 3H2 + Fe2(SO4)3Concentration (M of H2SO4)Reaction Time (seconds)1.000.000.1102.000.06254.000.02786.000.01568.000.010010.000.0117 mol/L*s17Discussion Questions6) As a reaction proceeds, the concentration of reactants will _______ and the concentration of products will ________.increase, decreaseincrease, increasedecrease, decreasedecrease, increaseD18Discussion Questions7) Calculate the rate of formation of iron(II) sulfide if sulfur is being consumed at a rate of 0.440 mol/Ls. 8 Fe(s) + S8(s) 8 FeS(s)3.52 mol/L*s19Discussion Questions8) Calculate the rate of formation of aluminum oxide if oxygen is being consumed at a rate of 0.060 mol/Ls. 3 O2(g) + 4Al(s) 2 Al2O3(s)0.040 mol/L*s20Discussion Questions9) At what rate is aluminum being consumed if aluminum oxide is being formed at 2.50 mol/Ls. 3 O2(g) + 4Al(s) 2 Al2O3(s)5.00 mol/L*s21Discussion Questions10) At what rate is nitrogen being consumed if hydrogen is being consumed at 0.0093 mol/Ls. 3 H2(g) + N2(g) 2 NH3(g)0.0031 mol/L*s22Other4597.5605