Consider the following reaction: 2NO(g)+2H2(g)N2(g)+2H2O(g). Part A The rate law
ID: 506381 • Letter: C
Question
Consider the following reaction:
2NO(g)+2H2(g)N2(g)+2H2O(g).
Part A
The rate law for this reaction is first order in H2 and second order in NO. Write the rate law.
Part B
If the rate constant for this reaction at 1000 K is 6.0×104M2s1, what is the reaction rate when [NO]= 4.00×102M and [H2]= 1.10×102M?
Express your answer using two significant figures and in M/s
Part C
What is the reaction rate at 1000 K when the concentration of NO is increased to 0.15 M, while the concentration of H2 is 1.10×102M?
Express your answer using two significant figures and in M/s
rate=k[H2][NO] rate=k[H2][NO]2 rate=k[H2]2[NO]2 rate=k[H2]Explanation / Answer
Rate = k*[H2]^a [ NO]^b
if [H2] = first order, then a = 1
if [NO] is second order, then b = 2
hence
Rate = k*[H2]^a [ NO]^b
Rate = k*[H2]^1 [ NO]^2
Rate = k*[H2][ NO]^2
B)
if K = 6*10^4 1/M2s, then find rate at
[NO] = 4*10^-2 and [H2] = 1.1*10^-2
simply
substitute in
Rate = k*[H2][ NO]^2
Rate = (6*10^4)*(1.1*10^-2)*(4*10^-2)^2
Rate 1.056 M/s
C
find rate when
[NO] increases to 0.15 M and [H2] = 1.1*10^-2
from
Rate = k*[H2][ NO]^2
Rate = (6*10^4)(1.1*10^-2)(0.15^2)
Rate = 14.85 M/s
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