Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
![The Rate Law
Review Questions
13.9
Explain what is meant by the rate law of a reaction.
13.10 What are the units for the rate constants of zero-
order, first-order, and second-order reactions?
13.11 Consider the zero-order reaction: A – product.
(a) Write the rate law for the reaction. (b) What are
the units for the rate constant? (c) Plot the rate of the
reaction versus [A].
13.12 On which of the following properties does the rate
constant of a reaction depend? (a) reactant concen-
trations, (b) nature of reactants, (c) temperature.
Problems
13.13 The rate law for the reaction
NH (aq) + NO, (aq) → N2(g) + 2H,O(1)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10f93153-1f0b-4e20-ae29-a2b30a5e29fe%2F66476011-45c0-4730-8a4f-9a4bb2d390b6%2F16q2pdq_processed.png&w=3840&q=75)
Transcribed Image Text:The Rate Law
Review Questions
13.9
Explain what is meant by the rate law of a reaction.
13.10 What are the units for the rate constants of zero-
order, first-order, and second-order reactions?
13.11 Consider the zero-order reaction: A – product.
(a) Write the rate law for the reaction. (b) What are
the units for the rate constant? (c) Plot the rate of the
reaction versus [A].
13.12 On which of the following properties does the rate
constant of a reaction depend? (a) reactant concen-
trations, (b) nature of reactants, (c) temperature.
Problems
13.13 The rate law for the reaction
NH (aq) + NO, (aq) → N2(g) + 2H,O(1)
![is given by rate = k[NH ][NO;]. At 25°C, the rate
constant is 3.0 x 10IM - s. Calculate the rate of the
reaction at this temperature if [NH ] = 0.26 M and
[NO] = 0.080 M.
13.14 Use the data in Table 13.2 to calculate the rate of
the reaction at the time when [F,] = 0.010 M and
[CIO:] = 0.020 M.
13.15 Consider the reaction
CARIS
A +B → products
From the following data obtained at a certain tem-
perature, determine the order of the reaction and
calculate the rate constant:
[A] (M) [B] (M)
Rate (M/s)
3.20 x 10"
3.20 x 10-
6.40 x 10"
1.50
1.50
1.50
2.50
3.00
1.50
13.16 Consider the reaction
ARIS
x + Y Z
From the following data, obtained at 360 K, (a) deter-
mine the order of the reaction, and (b) determine the
initial rate of disappearance of X when the concentra-
tion of X is 0.30 M and that of Y is 0.40 M.
Initial Rate of
Disappearance of X (M/s)
[X] (M) [Y] (M)
0.053
0.10
0.50
0.127
0.20
0.30
1.02
0.40
0.60
0.254
0.20
0.60
0.509
0.40
0.30
13.17 Determine the overall orders of the reactions to which
the following rate laws apply: (a) rate = k[NO,J°,
(b) rate = k, (c) rate = k[H2][Br2l, (d) rate =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10f93153-1f0b-4e20-ae29-a2b30a5e29fe%2F66476011-45c0-4730-8a4f-9a4bb2d390b6%2F1mmmu9n_processed.png&w=3840&q=75)
Transcribed Image Text:is given by rate = k[NH ][NO;]. At 25°C, the rate
constant is 3.0 x 10IM - s. Calculate the rate of the
reaction at this temperature if [NH ] = 0.26 M and
[NO] = 0.080 M.
13.14 Use the data in Table 13.2 to calculate the rate of
the reaction at the time when [F,] = 0.010 M and
[CIO:] = 0.020 M.
13.15 Consider the reaction
CARIS
A +B → products
From the following data obtained at a certain tem-
perature, determine the order of the reaction and
calculate the rate constant:
[A] (M) [B] (M)
Rate (M/s)
3.20 x 10"
3.20 x 10-
6.40 x 10"
1.50
1.50
1.50
2.50
3.00
1.50
13.16 Consider the reaction
ARIS
x + Y Z
From the following data, obtained at 360 K, (a) deter-
mine the order of the reaction, and (b) determine the
initial rate of disappearance of X when the concentra-
tion of X is 0.30 M and that of Y is 0.40 M.
Initial Rate of
Disappearance of X (M/s)
[X] (M) [Y] (M)
0.053
0.10
0.50
0.127
0.20
0.30
1.02
0.40
0.60
0.254
0.20
0.60
0.509
0.40
0.30
13.17 Determine the overall orders of the reactions to which
the following rate laws apply: (a) rate = k[NO,J°,
(b) rate = k, (c) rate = k[H2][Br2l, (d) rate =
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