Free Printable AP Chemistry Review: Kinetics

1.

What is the integrated rate law for a zero order reaction?

a)

ln[A]=-kt+ln[A]₀

b)

[A]=-kt+[A]₀

c)

$\frac{1}{\left[A\right]}$ =kt+ $\frac{1}{\left[A\right]}$ ₀

2.

What is the integrated rate law for a second order reaction?

a)

\frac{1}{\left[A\right]}

=kt+

\frac{1}{\left[A\right]}

₀

b)

[A]=-kt+[A]₀

c)

ln[A]=-kt+ln[A]₀

3.

What is the integrated rate law for a first order reaction?

a)

$\frac{1}{\left[A\right]}$ =kt+ $\frac{1}{\left[A\right]}$ ₀

b)

[A]=-kt+[A]₀

c)

ln[A]=-kt+ln[A]₀

4.

Which letter represents the activation energy?

a)

A

b)

B

c)

C

d)

D

e)

E

5.

Which letter
represent the intermediates?

a)

A

b)

B

c)

C

d)

D

e)

E

6.

Which letter represent the reactants?

a)

A

b)

B

c)

C

d)

D

e)

E

7.

Which letter represents the products?

a)

A

b)

B

c)

C

d)

D

e)

E

8.

Which letter represents the $\Delta H$ ?

a)

A

b)

B

c)

C

d)

D

e)

E

9.

Is this endothermic or exothermic?

a)

Endothermic

b)

Exothermic

10.

Hydrogen iodide decomposes according to the equation shown below. The second order rate constant for this reaction is $1.6x10^{-1}L\ mol^{-1}\ s\ ^{-1}$ at $700\degree C$ . If the initial concentration of HI in a container is $5.1x10^{-2}M$ , how many minutes will it take for the concentration to be reduced to $4.9x10^{-3}M$ at $700\degree C$ ?

a)

24.62 mins.

b)

123.25 mins.

c)

19.21 mins.

d)

44.62 mins.

11.

Which formula is used to calculate rate?

a)

$\frac{\Delta\left[A\right]}{\Delta t}$

b)

$\frac{\Delta t}{\Delta\left[A\right]}$

c)

$\frac{\left[A\right]}{t}$

12.

Which order of reaction is has a positive slope?

a)

first order

b)

second order

c)

zeroth order

13.

What is the order for the BrO3 ion?

a)

zeroth

b)

first

c)

second

14.

What is the order for the Br ion?

a)

zeroth

b)

first

c)

second

15.

What is the order of the H3O ion?

a)

zeroth

b)

first

c)

second

16.

What was the overall order?

(a)

17.

What is the rate law for the reaction?

a)

$\ln\left[A\right]=-kt+\ln\left[A\right]_o$

b)

$K=\frac{1.2}{\left[.1\right]^1\left[.1\right]^1\left[.1\right]^2}$

c)

$rate=K\left[BrO_3\right]^1\left[Br\right]^1\left[H_3O\right]^2$

18.

What is the overall reaction?

a)

$H_22ICl→2HCl+I_2$

b)

$H+ICl→HCl+I$

c)

$K\left[BrO_3\right]^1\left[Br\right]^1\left[H_3O\right]^2$

19.

What is/are the intermediates in the reaction?

a)

Pt

b)

H

c)

HCl

d)

I

20.

What is the catalyst in the reaction?

a)

H

b)

Pt

c)

HCl

d)

I

21.

What is the rate law based on the reaction mechanism?

a)

$K=\frac{\left[H_2\right]\left[2ICl\right]}{\left[2HCl\right]\left[I_2\right]}$

b)

$rate=K\left[A\right]\left[B\right]\left[C\right]$

c)

$rate=K\left[H_2\right]^1\left[ICl\right]^2$

AP Chemistry Review: Kinetics

Total questions: 21

Worksheet time: 11mins

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