End of Module 12 Quiz

Write a balanced reaction for which the following rate relationships are true.

1/2N2O5 → NO2 + O2
2 N2O5 → NO2 + 4 O2
2 N2O5 → 4 NO2 + O2
1/4NO2 + O2 → 1/2N2O5
4 NO2 + O2 → 2 N2O5

A rate is equal to 0.0200 M/s. If [A] = 0.100 M and rate = k[A]1, what is the new rate if the concentration of [A] is increased to 0.200 M?

0.0200 M/s 0.0200 M/s 0.0200 M/s
0.0400 M/s
0.0600 M/s
0.0800 M/s
0.100 M/s

Determine the rate law and the value of k for the following reaction using the data provided.

2 NO(g) + O2(g) → 2 NO2(g)

[NO]i (M) [O2]i (M) Initial Rate (M-1s-1)

0.030 0.0055 8.55 × 10-3

0.030 0.0110 1.71 × 10-2

0.060 0.0055 3.42 × 10-2

Rate = 3.1 × 105 M-3s-1[NO]2[O2]2
Rate = 1.7 × 103 M-2s-1[NO]2[O2]
Rate = 3.8 M-1/2s-1[NO][O2]1/2
Rate = 9.4 × 103 M-2s-1[NO][O2]2
Rate = 57 M-1s-1[NO][O2]

A rate is equal to 0.0200 M/s. If [A] = 0.100 M and rate = k[A]2[B]2, what is the new rate if the concentration of [A] is increased to 0.200 M?

0.0200 M/s
0.0400 M/s
0.0600 M/s
0.0800 M/s
0.100 M/s

What data should be plotted to show that experimental concentration data fits a first-order reaction?

ln(k) vs. Ea
ln[reactant] vs. time
ln(k) vs. 1/T
1/[reactant] vs. time
[reactant] vs. time

The rate constant for the first-order decomposition of N2O is 3.40 s-1. What is the half-life of the decomposition?

0.204 s 0.204 s
0.491 s
0.294 s
0.236 s
0.424 s

Carbon-14 has a half-life of 5720 years and this is a first-order reaction. If a piece of wood has converted 75% of the carbon-14, then how old is it?

4290 years
1430 years
2375 years
4750 years
11440 years

If the activation energy for a given compound is found to be 103 kJ/mol, with a frequency factor of 4.0 × 1013 s-1, what is the rate constant for this reaction at 398 K?

8.2 s-1
1.2 s-1
3.9 × 1010 s-1
1.7 × 1010 s-1
2.5 × 107 s-1

Which rate law is unimolecular?

Rate = k[A]2
Rate = k[A]
Rate = k[A][B][C]
Rate = k[A][B]
Rate = k[A]3

Given the following balanced equation, determine the rate of reaction with respect to [O2].

2 SO2(g) + O2(g) → 2 SO3(g)

Rate = -<img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/module-12_Q10_fig1.png" alt="" />
Rate = +1/4<img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/module-12_Q12_fig2.jpg" alt="" />
Rate= <img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/module-12_Q12_fig2.jpg" alt="" />
Rate= -1/3<img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/module-12_Q12_fig2.jpg" alt="" />

What are the units of k in the following rate law?

Rate = k[X][Y]1/2

M-1/2s
M-1s-12
M s
M-1s
M-1/2s-1

Which of the following represents the equation for a second-order half-life?

t 1/2 =
t1/2=
t1/2=
t 1/2 = [A]o
t1/2=

Which of the following represents the integrated rate law for a zeroth-order reaction?

k = Ae(-Ea/RT)
<img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/Module12_Quiz_fig12.png" alt="" />
A]t – [A]o = – kt
<img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/Module12_Quiz_fig13.png" alt="" />

Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled?

Rate = k[X][Y]2

The rate of reaction will increase by a factor of 2.
The rate of reaction will decrease by a factor of 2.
The rate of reaction will increase by a factor of 4.
The rate of reaction will increase by a factor of 1/2.
The rate of reaction will remain unchanged.

What are the units of k in the following rate law?

Rate = k[X] [Y]3

<img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/module-12_Q15_fig2.jpg" alt="" />
<img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/module-12_Q15_fig3.jpg" alt="" />
M s2
<img src="https://gsuprincipleschemistry.org/wp-content/uploads/2023/05/module-12_Q15_fig4.jpg" alt="" />

Given the following balanced equation, determine the rate of reaction with respect to [Cl2]. If the rate of Cl2 loss is 4.24 × 10-2 M/s, what is the rate of formation of NOCl?

2 NO(g) + Cl2(g) → 2 NOCl(g)

1.61 × 10-2 M/s
4.24 × 10-2 M/s
2.12 × 10-2 M/s
8.48 × 10-2 M/s
1.06 × 10-1 M/s

If the concentration of a reactant is 6.25%, how many half-lives has it gone through?

3
10
4
7
5

The isomerization of methylisonitrile to acetonitrile

CH3NC(g) → CH3CN(g)

is first order in NC. The half-life of the reaction is 5.20 × 101 s at 545 K. The rate constant when the initial [NC] is 0.030 M is ________ .

2.84 × 104
0.0133
1.56
75.1
0.641

The second-order reaction 2 Mn(CO)5 → Mn2(CO)10, has a rate constant equal to 3.0 × 109 M-1 s-1 at 25°C. If the initial concentration of Mn(CO)5 is 2.0 × 10-5 M, how long will it take for 90.% of the reactant to disappear?

6.7 × 10-16 s
6.0 × 103 s
1.5 × 10-4 s
7.4 × 10-15 s

Given the following proposed mechanism, predict the rate law for the overall reaction.

2 NO2 + Cl2 → 2 NO2Cl (overall reaction)

Mechanism

NO2 + Cl2 → NO2Cl + Cl slow

NO2 + Cl → NO2Cl fast

Rate = k[NO2Cl]2[Cl]
Rate = k[NO2Cl][Cl]
Rate = k[NO2] [Cl]2
Rate = k[NO2]2[Cl2]2
Rate = k[NO2][Cl2]

CHEM 1212

End of Module 12 Quiz

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