The reaction 2 NO(g) + 2 H 2 (g) --> N 2 (g) + 2 H 2 O(g) proceeds through the f
ID: 884072 • Letter: T
Question
The reaction 2 NO(g) + 2 H2(g) --> N2(g) + 2 H2O(g) proceeds through the following mechanism:
2 NO(g) --> N2O2(g)
N2O2(g) + H2(g) --> H2O(g) + N2O(g)
N2O(g) + H2(g) --> N2(g) + H2O(g)
(a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction?
Rate = k [NO] [H2] Rate = k [NO]2 [H2]
Rate = k [NO] [H2]2 Rate = k [NO]1/2 [H2]
Rate = k [NO] [H2]1/2
Rate = k [NO]2
Rate = k [NO]2 [H2]1/2
(b) What would the rate law be if the first step of this mechanism were rate-determining?
Rate = k [NO] [H2] Rate = k [NO]2 [H2]
Rate = k [NO] [H2]2
Rate = k [NO]1/2 [H2]
Rate = k [NO] [H2]1/2
Rate = k [NO]2
Rate = k [NO]2 [H2]1/2
Rate = k [NO]
Explanation / Answer
For a general reaction
aA + bB = products
The rate equation is Rate = k [A]a [B]b
(a) The second step is
N2O2(g) + H2(g) --> H2O(g) + N2O(g)
which is the rate determining step
The rate law is
Rate = k [N2O2][ H2]
Since N2O2 = 2 NO, the rate law can be rewrtten as
Rate = k [NO]2 [ H2]
(b) The first step is 2 NO(g) --> N2O2(g)
The rate law is
Rate = k [NO]2
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