Question

1. Why does increasing the temperature increase the rate of a chemical reaction?

a.The molecules are colliding with the walls of the container more often.

b.The products of the reaction act as a catalyst, increasing the rate of reaction.

c.There are more collisions between molecules, and the collisions have more energy.

d.The products are formed more rapidly, increasing the reactivity of the system.

2. Using the data in the following table, calculate the average rate of the reaction

2NO2(g) → 2NO(g) + O2(g).

Time(s) [NO2]

0 0.125

520 0.098

a. 1.9 × 10-4 M/s

b. 2.4 × 10-4 M/s

c. 5.2 × 10-5 M/s

d. 2.6 × 10-5 M/s

3. Chlorine dioxide is a reddish yellow gas that dissolves in water. In basic solution this reaction takes place:

2ClO2(aq) + 2OH- (aq) → ClO2- (aq) + ClO3- (aq) + H2O(l).

Based on the following data, determine the rate law and the value of the rate constant.

Initial Concentrations Initial Rate

[ClO2] [OH-] (M/s

0.060 0.030 0.0248

0.020 0.030 0.00276

0.020 0.090 0.00828

What is the rate law and rate constant for this reaction?

a. rate = 6.9M-1s-1[ClO2]2

b. rate = 14M-1s-1[ClO2][OH]

c. rate = 230M-2s-1[ClO2]2[-OH]

d. rate = 0.83s-1[OH]

4. The hydrolysis of t-butyl chloride in an organic solvent occurs by the reaction

(CH3)3CBr(g) + H2O(g) → (CH3)3OH(g) + HBr(g).

The rate law is rate = k [(CH3)3CBr].

How would the initial rate change if the concentration of water is doubled?

a. The initial rate would not change.

b. The initial rate would double.

c. The initial rate would increase by a factor of four.

d. The initial rate would increase by a factor of three.

5. The decomposition of N2O5 is first order in N2O5 and proceeds with a rate constant of 5.0 × 10-4 sec-1. What is the half-life of this reaction?

a. 2000 sec

b. 2900 sec

c. 5800 sec

d. 1400 sec

Answer 1