Consider the following reaction: Q:4-1 2 NO(g) + 2 H2(8) → N;(g) + 2 H,O(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 × 10ª M¯²s¯1, what is the re- action rate when [NO] = 0.035 M and [H,] = 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 [H] is increased to 0.030 M?

Consider the following reaction: Q:4-1 2 NO(g) + 2 H2(8) → N;(g) + 2 H,O(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 × 10ª M¯²s¯1, what is the re- action rate when [NO] = 0.035 M and [H,] = 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 [H] is increased to 0.030 M?

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

Q:4-1
Consider the following reaction:
2 NO(g) + 2 H2(8) → N;(g) + 2 H,O(g)
(a) The rate law for this reaction is first order in H, and second
order in NO. Write the rate law. (b) If the rate constant for
this reaction at 1000 K is 6.0 × 10ª M¯²s¯!, what is the re-
action rate when [NO] = 0.035 M and [H,] = 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 H,
is 0.010 M? (d) What is the reaction rate at 1000 K if [NO] is
decreased to 0.010 M and [H,] is increased to 0.030 M?
%3D
Q:4-2
The iodide ion reacts with hypochlorite ion (the ac-
tive ingredient in chlorine bleaches) in the following way:
OCI- + I- –→ OI¯ + Cl¯. This rapid reaction gives the
following rate data:
[OCI¯] (M)
[I-] (M)
Initial Rate (M/s)
1.5 X 10-3
1.5 X 10¬3
1.36 X 10¬4
3.0 × 10–3
1.5 X 10–3
2.72 X 10¬4
1.5 × 10-3
3.0 × 10-3
2.72 X 10¬4
(a) Write the rate law for this reaction. (b) Calculate the
rate constant with proper units. (c) Calculate the rate when
[OCI] = 2.0 × 10-³ M and [I¯] = 5.0 × 10-4 M.

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