1. The initial velocity of the gas-phase PNo (atm) 0.090 Рнг (atm) Vo (atm/s of N2) 8.4 x 10 4.2 x 10" reaction 0.030 k 0.015 0.090 2 H2 + 2 NO → 2 H20 + N2 0.030 0.045 2.1 x 107 was studied at 700 °C. Data in the table at right shows the initial rate of reaction under different reaction concentration conditions. a) What is the order of this reaction for PNo? Explain. b) Write down the rate law for this reaction based on the data in the table. (This is a formula.) c) In the formula of part b), what is the value of the rate constant k? (This is a number.)
1. The initial velocity of the gas-phase PNo (atm) 0.090 Рнг (atm) Vo (atm/s of N2) 8.4 x 10 4.2 x 10" reaction 0.030 k 0.015 0.090 2 H2 + 2 NO → 2 H20 + N2 0.030 0.045 2.1 x 107 was studied at 700 °C. Data in the table at right shows the initial rate of reaction under different reaction concentration conditions. a) What is the order of this reaction for PNo? Explain. b) Write down the rate law for this reaction based on the data in the table. (This is a formula.) c) In the formula of part b), what is the value of the rate constant k? (This is a number.)
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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Transcribed Image Text:1. The initial velocity of the gas-phase
PNo (atm)
0.090
Рнг (atm)
Vo (atm/s of N2)
8.4 x 10
4.2 x 10"
reaction
0.030
k
0.015
0.090
2 H2 + 2 NO → 2 H20 + N2
0.030
0.045
2.1 x 107
was studied at 700 °C. Data in the table at right shows the initial rate of reaction under different
reaction concentration conditions.
a) What is the order of this reaction for PNo? Explain.
b) Write down the rate law for this reaction based on the data in the table. (This is a formula.)
c) In the formula of part b), what is the value of the rate constant k? (This is a number.)
d) Shown at right is a set of elementary reactions that
make up the proposed mechanism for this reaction. What
is the value of the rate constant in part b) in terms of the
equilibrium and rate constants (K2 and ki) in the
elementary reactions? (This is a formula.)
ki
H2 + 2 NO - N2 + H20 + Q slow
K2
O+ H2 H2O,
fast
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