Chemistry Review Name: _______________________________Chapter 13 Chemical Kinetics Date: ____________ Period: ____________

1. All of the following factors affect the initial rate of a reaction except?

A) the nature of the reactantsB) the temperatureC) a catalyst D) the concentration of the productsE) the concentration of the reactants

2. In the reaction

2 NO2 2 NO + O2

at 300oC, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate of appearance of O2 for this period is ____________ M/s.

A) 0.0000175 B) 0.0000350 C) 0.0000700 D) 0.00350 E) 0.00700

3. The reaction that occurs in a Breathalyzer, a device used to determine the alcohol level in a person’s bloodstream, is given below. If the rate of appearance of Cr2(SO4)3 is 1.24 mol/min at a particular moment, what is the rate of disappearance of C2H6O at that moment?

2 K2Cr2O7 + 8 H2SO4 + 3 C2H6O 2 Cr2(SO4)3 + K2SO4 + 11 H2O

A) 3.72 mol/min B) 0.413 mol/min C) 0.826 mol/min D) 1.86 mol/min E) 1.652 mol/min

4. The decomposition of dinitrogen pentoxide is described by the chemical equation:

2 N2O5 (g) 4 NO2 (g) + O2 (g)

If the rate of disappearance of N2O5 is equal to 1.40 mol/min at a particular moment, what is the rate of appearance of NO2 at that moment?

A) 1.40 mol/min B) 2.80 mol/min C) 5.60 mol/min D) 0.700 mol/min

5. From a consideration of the gaseous reaction

aA + bB cC + dD Rate = k[A]q[B]r

Which of the following is false?

A) The exponents q and r are likely to be integers. B) The exponents q and r are always equal to the coefficients a and b respectively. C) The exponents q and r must be determined experimentally. D) The symbol k represents the rate constant. E) The overall reaction order is q + r.

6. The rate law, R = k[NO]2[Br], is given for the following reaction 2 NO (g) + Br2 2 NOBr (g). What is the overall order of the reaction.

A) 0 B) 1 C) 2 D) 3 E) 4

7. A reaction is discovered to have the following rate law. Rate = k [NO2]2 . If the concentration of NO2 is tripled, the rate of the reaction will

A) stay the same. B) double. C) triple. D) quadruple. E) go up by 9.

8. The following set of data was obtained by the method of initial rates for the reaction:

2 HgCl2 (aq) + C2O42- (aq) 2 Cl- (aq) + 2 CO2 (g) + Hg2Cl2 (s)

What is the rate law for the reaction?

[HgCl 2] [C2O42- ] Rate, M/s

0.10 0.10 1.3 x 10-7

0.10 0.20 5.2 x 10-7

0.20 0.20 1.0 x 10-6

A) Rate = k[HgCl2]2[C2O42-]

B) Rate = k[HgCl2][C2O42-]2

C) Rate = k[HgCl2][C2O42-]-2

D) Rate = k[HgCl2][C2O42-]-1

9. What is the value of k from the question above?

A) 1.3 x 10-7

B) 1.4 x 10-8

C) 1.4 x 10-5

D) 1.3 x 10-4

10. Given the data below for the reaction:

2Y + 3Z products

the rate law is R = _______________.

[Y] [Z] Initial Rate, M/s0.100 0.100 4.0 x 10-5

0.200 0.100 1.6 x 10-4

0.100 0.200 8.0 x 10-5

A) Rate = k[Y][Z]B) Rate = k[Y]2[Z]

C) Rate = k[Y]2[Z]2

D) Rate = k[Y][Z]2

E) Rate = k[Y]-1[Z]2

11. The following set of data was obtained by the method of initial rates for the reaction:

(H3C)3CBr + OH- (H3C)3COH + Br-

What is the value of the rate constant, k?

[(H3C)3CBr] [OH - ] Initial Rate, M/s0.25 0.25 1.1 x 10-4

0.50 0.25 2.2 x 10-4

0.50 0.50 2.2 x 10-4

A) 1.8 x 10-4 B) 4.4 x 10-4

C) 8.8 x 10-4

D) 3.6 x 10-4

E) None of these

12. For a particular first-order reaction, it takes 48 minutes for the concentration of the reactant to decrease to 25% of its initial value. What is the value for the rate constant (in s-1) for the reaction?

A) 6.0 x 10-3 s-1

B) 4.8 x 10-4 s-1

C) 1.0 x 10-4 s-1

D) 2.9 x 10-2 s-1

E) None of these

13. The isomerization reaction of CH3NC CH3CN, is first order and the rate constant is equal to 0.46 s-1 at 600K. What is the concentration of CH3NC after 0.20 minutes if the initial concentration is 0.10 M?

A) 4.0 x 10-2 M B) 4.0 x 10-4 MC) 9.1 x 10-4 M D) 9.1 x 10-2 M E) None of these

14. Acetaldehyde decomposes at 790 K: CH3CHO CO + CH4. The reaction is first order in acetaldehyde and the half-life of the reaction is found to be 530 seconds. What is the rate constant for the reaction at this temperature?

A) 2.7 x 102 s-1

B) 7.6 x 102 s-1

C) 2.7 x 10-3 s-1

D) 1.3 x 10-3 s-1

E) None of these

15. The first-order reaction, SO2Cl2 SO2 + Cl2, has a half-life of 8.75 hours at 593 K. How long will it take for the concentration of SO2Cl2 to fall to 12.5% of its initial value?

A) 26.2 hours B) 3.22 hoursC) 0.165 hours D) 28.3 hours E) None of these

16. The second-order reaction, 2 Mn(CO)5 Mn2(CO)10 has a rate constant equal to 3.0 x 109 M-1s-1 at 25oC. If the initial concentration of Mn(CO)5 is 1.0 x 10-5 M, how long will it take for 90% of the reactant to disappear?

A) 3.0 x 10-4 s B) 3.3 x 10-16 sC) 3.0 x 103 s D) 3.7 x 10-15 s E) None of these

17. A certain radioactive decay process (1st order) is 45% complete in 65 sec. What is the half-life for this process?

A) t1/2 = 74 s B) t1/2 = 12 sC) t1/2 = 85 sD) t1/2 = 56 sE) None of these

18. The rate constant for a reaction is 1.3 M-1s-1 at 700 K and 23 M-1s-1 at 800 K. What is the activation energy?

A) 157 KJ B) 67 KJC) 143 KJD) 133 KJE) None of these

19. A reaction occurs by the steps given below? Which rate law is consistent with this mechanism?

2 NO (g) N2O2 (g) fastN2O2 (g) + H2 (g) 2 N2O (g) + H2O (g) slow N2O (g) + H2 (g) N2 (g) + H2O (g) fast

A) Rate = k[N2O2][H2]B) Rate = k[NO]2[N2O2][H2]C) Rate = k[NO]2[H2]D) Rate = k[NO][H2]E) None of these

20. A proposed two-step mechanism is

NO2 (g) + NO2 (g) NO3 (g) + NO (g) [Slow]NO3 (g) + CO (g) NO2 (g) + CO2 (g) [Fast]

Identify the reaction intermediate.

A) NO2

B) NO3

C) NOD) COE) CO2

21. A catalyst works by:

A) Increasing the H of the reaction.B) Decreasing the temperature of the reaction. C) Decreasing the energy of the reactants. D) Decreasing the differences in the energies of products vs. reactants. E) Decreasing the activation energy of the rate determining step.

22. After three half-lives have gone by:

A) all of the reactant has been changed to product. B) 87.5% of the reactant has been changed to product. C) 75% of the reactant has been changed to product.D) 50% of the reactant has been changed to product.E) 12.5% of the reactant has been changed to product.

23. If a reaction is 1st order, a plot of _____ as function of _____will yield a straight line?

A) [A]t, [A]0

B) [A]t, timeC) 1/[A]t, time D) ln[A]t, time E) None of these

24. A reaction with the activation energy Ea= 219.00 kJ/mol, has a rate constant k = 1.400 x 102 at 988.00 Kelvin. Determine the rate constant when the temperature is changed to 238.00 Kelvin.

25. A reaction with the activation energy Ea= 92.00 kJ/mol, has a rate constant k = 8.500 x 10-4 at 379.00 Kelvin. Determine the temperature required to increase the rate constant 5 times.

Chemistry Review Name: _______________________________Chapter 14 Chemical Equilibrium Date: ____________ Period: ____________

1. Write the equilibrium equation for each of the following reactions:

a. N2(g) + 3 H2(g) ↔ 2 NH3(g)

b. NH4Cl(s) ↔ NH3(g) + HCl(g)

c. CaCO3(s) ↔ CaO(s) + CO2(aq)

2. A mixture of 9.22 moles of A, 10.11 moles of B, and 27.83 moles of C is placed in a one-litercontainer at a certain temperature. The reaction is allowed to reach equilibrium. At equilibrium the number of moles of B is 18.32. Calculate the equilibrium constant for the reaction:

A (g) + 2 B (g) ↔ 3 C (g)

3. For the reaction 2CO(g) ↔ C(s) + CO2(g), Keq = 7.7 x 10-15. At a particular time, the following concentrations are measured: [CO]=0.034 M, [CO2] =3.6x10-17M. Is this reaction at equilibrium? If not which direction will the reaction proceed?

4. For the reaction 2ICl(g) ↔ I2(g) + Cl2(g), Keq = 0.11. At a particular time, the following concentrations are measured: [ICl]=2.5 M, [I2] =2.0 M, [Cl2]= 1.2 M. Is this reaction at equilibrium? If not which direction will the reaction proceed?

5. The equilibrium constant for the reaction: 2 NO (g) ↔ N2 (g) + O2 (g) is 2.60 x 10-3 at 1100 °C. If 0.820 mole of NO (g) and 0.223 mole each of N2 (g) and O2 (g) are mixed in a 1.00 liter container at 1100 °C, what are the concentrations of NO (g), N2(g), and O2 (g) at equilibrium?

6. Use Le Chatelier’s principle to predict how the changes listed will affect the concentration of HI for thefollowing equilibrium reaction: 2HI(g) ↔ H2(g) + I2(g) ∆H = 9.4 kJ

a small amount of H2 is added.b. the pressure of the system is increased.c. the temperature of the system is increased.d. a catalyst is added.

7.