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12. Basic Chemistry: Chemical Kinetics

Total questions: 25

Worksheet time: 2hrs 9mins

Name
Class
Date
1.

Which of the following is NOT a factor affecting reaction rate?

a)
Temperature of the reactants
b)
Concentration of the reactants
c)
Presence of a catalyst
d)
Surface area of the reactants
e)

Polarity of the reactants

2.

The catalyst alters the rate of a chemical reaction by .......................

a)
increasing the temperature
b)

changing the products formed in the direction of the reaction

c)

providing an alternative pathway with a lower Ea

d)

increasing the frequencies of collisions between molecules

e)

providing a surface on which the molecules react

3.

Which of the following are true about reaction rates?

a)

The overall rate law is determined by the fastest step of a reaction.

b)

The presence of a catalyst will increase the number of molecules entering the transition state.

c)

An increase in temperature will increase the rate of a reaction.

d)

Decreasing the particle size will make particles move faster.

e)

Decreasing the concentration of reactants will increase the rate at which products yield.

4.

To measure rate of reaction, we can monitor change in which of the following?

a)

concentration reactants or products

b)

colour of products

c)

mass product

d)

pH level of reactant

e)

temperature product

5.

The rate of reaction is the change in the ............ of a reactant or product per unit of ...............

a)

temperature, pressure.

b)

mass, concentration.

c)

pressure, time.

d)

concentration, time.

e)

mass, temperature.

6.

2N2O5(g) → 4NO2(g) + O2(g)

rate of following reaction is ........................

a)

rate =−12×Δ[N2O5]Δt=14×Δ[NO2]Δt=Δ[O2]Δtrate\ =-\frac{1}{2}\times\frac{\Delta\left[N_2O_5\right]}{\Delta t}=\frac{1}{4}\times\frac{\Delta\left[NO_2\right]}{\Delta t}=\frac{\Delta\left[O_2\right]}{\Delta t}

b)

rate =−1×Δ[N2O5]Δt=2×Δ[NO2]Δt=12Δ[O2]Δtrate\ =-1\times\frac{\Delta\left[N_2O_5\right]}{\Delta t}=2\times\frac{\Delta\left[NO_2\right]}{\Delta t}=\frac{1}{2}\frac{\Delta\left[O_2\right]}{\Delta t}

c)

rate =−14×Δ[N2O5]Δt=12×Δ[NO2]Δt=1×Δ[O2]Δtrate\ =-\frac{1}{4}\times\frac{\Delta\left[N_2O_5\right]}{\Delta t}=\frac{1}{2}\times\frac{\Delta\left[NO_2\right]}{\Delta t}=1\times\frac{\Delta\left[O_2\right]}{\Delta t}

d)

rate =−12×Δ[NO2]Δt=14×Δ[N2O5]Δt=1×Δ[O2]Δtrate\ =-\frac{1}{2}\times\frac{\Delta\left[NO_2\right]}{\Delta t}=\frac{1}{4}\times\frac{\Delta\left[N_2O_5\right]}{\Delta t}=1\times\frac{\Delta\left[O_2\right]}{\Delta t}

e)

rate =−12×Δ[O2]Δt=14×Δ[N2O5]Δt=1×Δ[NO2]Δtrate\ =-\frac{1}{2}\times\frac{\Delta\left[O_2\right]}{\Delta t}=\frac{1}{4}\times\frac{\Delta\left[N_2O_5\right]}{\Delta t}=1\times\frac{\Delta\left[NO_2\right]}{\Delta t}

7.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the order in [BF3] ?

a)

1

b)

0

c)

3

d)

4

e)

2

8.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the order in [NH3] ?

a)

4

b)
2
c)
1
d)
0
e)
3
9.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate constant (k) of the reaction?

a)

0.625

b)

0.213

c)

2.596

d)

3.408

e)

1.193

10.

The following data were measured for the reaction

BF3(g) + NH3(g) ⟶ F3BNH3(g)

What is the rate when [BF3] = 0.100 M and [NH3] = 0.500 M ?

a)

0.1704 M/s

b)

0.852 M/s

c)

0.0625 M/s

d)

0.3125 M/s

e)

0.0852 M/s

11.

A reaction is found to be second order with respect to carbon monoxide. If the concentration of carbon monoxide is doubled, the rate of reaction ...........

a)
remains the same
b)
decreases by a factor of 2
c)
increases by a factor of 3
d)
increases by a factor of 4
e)
increases by a factor of 1
12.

Given the following rate law, rate = k[A]2[B]. If [A] were doubled, what must happen to [B] to keep the rate constant?

a)
[B] must be doubled.
b)
[B] must remain the same.
c)
[B] must be reduced to one-fourth of its original concentration.
d)
[B] must be increased to four times its original concentration.
e)
[B] must be halved.
13.

Rate = k[A]. The rate constant in the rate law above is 0.5 L/mol·s. If the initial concentration of A is 0.1 M, how long will it take for [A] to drop to 0.025 M?

a)
5.000 seconds
b)
1.500 seconds
c)
3.500 seconds
d)
2.772 seconds
e)
4.000 seconds
14.

Given the following balanced equation :

2NO(g) + Cl2(g) → 2NOCl(g)

If the rate of disappearance of Cl2 is 4.84 x 10-2 Ms-1, what is the rate of disappearance of NO?

a)

1.22 x 10-1 M/s

b)

4.84 x 10-2 M/s

c)

9.68 x 10-2 M/s

d)

2.42 x 10-2 M/s

e)

8.00 x 10-2 M/s

15.

The first order rate constant for the decomposition of 0.5 M compound A at 100oC is 0.03 min-1. Calculate the half-life of A.

a)
30.2 minutes
b)
5.0 minutes
c)
15.4 minutes
d)
10.5 minutes
e)
23.1 minutes
16.

In the reaction 2O₃ (g) → 3O₂ (g), what is the relative rate expression for O₃?

a)

2 x (Δ[O₃]/Δt)

b)

-3 x (Δ[O₃]/Δt)

c)

-1/3 x (Δ[O₃]/Δt)

d)

-1/2 x (Δ[O₃]/Δt)

e)

1/2 x (Δ[O₃]/Δt)

17.

In the reaction 2O₃ (g) → 3O₂ (g), what is the relative rate expression for O₂?

a)
Rate of O₂ = (1/2) * Rate of O₃
b)
Rate of O₂ = (3/4) * Rate of O₃
c)
Rate of O₂ = (3/2) * Rate of O₃
d)
Rate of O₂ = Rate of O₃
e)
Rate of O₂ = (2/3) * Rate of O₃
18.

Which of the following statements is true regarding the order of a reaction?

a)

The order of a reaction must be determined experimentally.

b)
The order of a reaction is determined solely by temperature.
c)
The order of a reaction is the sum of the powers of the concentration terms in the rate law.
d)

The order of a reaction is always equal to the stoichiometric coefficients in the balanced equation.

e)
The order of a reaction can never be zero.
19.

A reaction is found to have an activation energy of 108 kJ/mol. If the rate constant for this reaction is 4.60×10−6/s at 275 K, what is the rate constant at 366 K? R = 8.314 J/mol.K. 1 kJ = 1000 J

a)
0.136 /s
b)

0.580 /s

c)
0.075 /s
d)
0.250 /s
e)
0.045 /s
20.

For first order reaction A → product, the initial concentration of A is 0.1 M. After 40 minutes, the concentration of A becomes 0.025 M. What is the rate of reaction at reactant concentration 0.01 M?

a)

1.25 x 10-4 M/min

b)

5.00 x 10-4 M/min

c)

3.47 x 10-4 M/min

d)

6.93 x 10-4 M/min

e)

1.73 x 10-4 M/min

21.

For the reaction 2N2O5(g) → 4NO2(g) + O2(g), the concentration of NO2 increase by 2.4 x 10-2 M in 6 seconds. What will be the average rate of appearance of NO2 and the average rate of disappearance of N2O5?

a)

2.0 x 10-3 M/s and 4.0 x 10-3 M/s

b)

2.0 x 10-3 M/s and 1.0 x 10-3 M/s

c)

4.0 x 10-3 M/s and 2.0 x 10-3 M/s

d)

2.0 x 10-3 M/s and 2.0 x 10-3 M/s

e)

6.0 x 10-3 M/s and 2.0 x 10-3 M/s

22.

The rate of a reaction is approximately doubled for every 10°C rise in temperature. If temperature rise by 50°C, the reaction rate increase by about ......................

a)
64 times
b)
16 times
c)
32 times
d)
8 times
e)
4 times
23.

The iodide ion reacts with hypochlorite ion in the following way:

OCl- + I- ⟶ OI- + Cl-.

This rapid reaction gives the rate data shown. What is the rate law?

a)

rate = k[OCl-][I-]

b)

rate = k[OCl-][I-]2

c)

rate = k[OCl-]2[I-]

d)
rate = k[I-]
e)
rate = k[OCl-]
24.

What would the rate constant of the reaction be given the following set of experiments?

a)

k = 0.517 /Ms

b)

k = 0.138 /Ms

c)

k = 0.179 /Ms

d)

k = 0.275 /Ms

e)

k = 0.266 /Ms

25.

An addition of a catalyst to the following reaction would have what effect?

a)

A would be increased

b)

B would be increased

c)

C would be increased

d)

B would be decrease

e)

No change

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