The reaction of nitric oxide with hydrogen at 1280°C is 2NO(3) + 2H;(3) ► N;(8) + 2H,0(g) From the following data collected at this temperature, determine (a) the rate law, (b) the rate constant, and (c) the rate of the reaction when [NO] = 12.0 × 10 M and (H;) = 6.0 × 10"' M. [NO] (M) 5.0 x 10-3 10.0 x 10-3 10.0 x 10-3 [H;] (M) 2.0 x 10-3 2.0 x 10-3 4.0 x 10-3 Experiment Initial Rate (M/s) 1.3 x 10-5 5.0 x 10-5 10.0 x 10-5 2 3 Strategy We are given a set of concentration and reaction rate data and asked to determine the rate law and the rate constant. We assume that the rate law takes the form rate = k{NO}{|H;P" %3D
The reaction of nitric oxide with hydrogen at 1280°C is 2NO(3) + 2H;(3) ► N;(8) + 2H,0(g) From the following data collected at this temperature, determine (a) the rate law, (b) the rate constant, and (c) the rate of the reaction when [NO] = 12.0 × 10 M and (H;) = 6.0 × 10"' M. [NO] (M) 5.0 x 10-3 10.0 x 10-3 10.0 x 10-3 [H;] (M) 2.0 x 10-3 2.0 x 10-3 4.0 x 10-3 Experiment Initial Rate (M/s) 1.3 x 10-5 5.0 x 10-5 10.0 x 10-5 2 3 Strategy We are given a set of concentration and reaction rate data and asked to determine the rate law and the rate constant. We assume that the rate law takes the form rate = k{NO}{|H;P" %3D
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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Answer example 13.3 and include what's given and required, also use cancellations if possible. By using rate law.
![4PH;(8)
PA(8) + 6H;(8).
Suppose that, at a particular moment during the reaction, molecular hydrogen is being
formed at the rate of 0.078 Mls. (a) At what rate is P, being formed? (b) At what rate
is PH; reacting?
13.2 The Rate Law
So far we have learned that the rate of a reaction is proportional to the concentration
of reactants and that the proportionality constant k is called the rate constant. The rate
law expresses the relationship of the rate of a reaction to the rate constant and the
concentrations of the reactants raised to some powers. For the general reaction
aA + bB – CC + dD
the rate law takes the form
rate = k[A]'[B]
(13.1)
where x and y are numbers that must be determined experimentally. Note that, in
general, x and y are not equal to the stoichiometric coefficients a and b. When we
EXAMPLE 13.3
The reaction of nitric oxide with hydrogen at 1280°C is
2NO(3) + 2H;(g)
→ N(8) + 2H,0(3)
From the following data collected at this temperature, determine (a) the rate law,
(b) the rate constant, and (c) the rate of the reaction when [NO] = 12.0 × 10~³ M and
[H;] = 6.0 × 10"³ M.
[NO] (M)
5.0 X 10
10.0 × 10-3
10.0 × 10~3
[H;] (M)
2.0 × 10-3
2.0 × 10-3
4.0 x 10-3
Experiment
Initial Rate (M/s)
1.3 × 10-$
5.0 × 10-5
10.0 × 10~5
1
3
Strategy We are given a set of concentration and reaction rate data and asked to
determine the rate law and the rate constant. We assume that the rate law takes the
form
rate = k[NO]"[H;P'](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd5b05f87-cc99-48cd-ba35-706717ce0324%2F4b8b9d66-eab6-4829-a9eb-251efafcd709%2F2rgyb6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:4PH;(8)
PA(8) + 6H;(8).
Suppose that, at a particular moment during the reaction, molecular hydrogen is being
formed at the rate of 0.078 Mls. (a) At what rate is P, being formed? (b) At what rate
is PH; reacting?
13.2 The Rate Law
So far we have learned that the rate of a reaction is proportional to the concentration
of reactants and that the proportionality constant k is called the rate constant. The rate
law expresses the relationship of the rate of a reaction to the rate constant and the
concentrations of the reactants raised to some powers. For the general reaction
aA + bB – CC + dD
the rate law takes the form
rate = k[A]'[B]
(13.1)
where x and y are numbers that must be determined experimentally. Note that, in
general, x and y are not equal to the stoichiometric coefficients a and b. When we
EXAMPLE 13.3
The reaction of nitric oxide with hydrogen at 1280°C is
2NO(3) + 2H;(g)
→ N(8) + 2H,0(3)
From the following data collected at this temperature, determine (a) the rate law,
(b) the rate constant, and (c) the rate of the reaction when [NO] = 12.0 × 10~³ M and
[H;] = 6.0 × 10"³ M.
[NO] (M)
5.0 X 10
10.0 × 10-3
10.0 × 10~3
[H;] (M)
2.0 × 10-3
2.0 × 10-3
4.0 x 10-3
Experiment
Initial Rate (M/s)
1.3 × 10-$
5.0 × 10-5
10.0 × 10~5
1
3
Strategy We are given a set of concentration and reaction rate data and asked to
determine the rate law and the rate constant. We assume that the rate law takes the
form
rate = k[NO]"[H;P'
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