Consider the following reaction:2 NO(g) + 2 H2(g)--->N2(g) + 2 H2O(g)(a) The rate law for this reaction is first order in H2 andsecond order in NO. Write the rate law. (b) If the rateconstant for this reaction at 1000 K is 6.0 x 104 M-2 s-1,what is the reaction rate when [NO] = 0.035 M and[H2] = 0.015 M? (c) What is the reaction rate at 1000 Kwhen the concentration of NO is increased to 0.10 M,while the concentration of H2 is 0.010 M? (d) What is thereaction rate at 1000 K if [NO] is decreased to 0.010 M and[H2] is increased to 0.030 M?

a) Since the rate of reaction depends only on the reactant concentration and the order of reaction…

Answered: Consider the following reaction:2 NO(g)…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section: Chapter Questions

Problem 24PS: Hydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is...

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Consider the following reaction:
2 NO(g) + 2 H₂(g)--->N₂(g) + 2 H₂O(g)
(a) The rate law for this reaction is first order in H₂ and
second order in NO. Write the rate law. (b) If the rate
constant for this reaction at 1000 K is 6.0 x 10⁴ M^-2 s^-1,
what is the reaction rate when [NO] = 0.035 M and
[H₂] = 0.015 M? (c) What is the reaction rate at 1000 K
when the concentration of NO is increased to 0.10 M,
while the concentration of H₂ is 0.010 M? (d) What is the
reaction rate at 1000 K if [NO] is decreased to 0.010 M and
[H₂] is increased to 0.030 M?

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