The reaction, 2 NO(g) + 2 H 2 (g)--> N 2 (g) + 2 H 2 O(g), proceedsthrough the f

Question

The reaction, 2 NO(g) + 2 H2(g)--> N2(g) + 2 H2O(g), proceedsthrough the following mechanism:

2 NO(g) -->N2O2(g)
N2O2(g) +H2(g) --> H2O(g) +N2O(g)
N2O(g) + H2(g) -->N2(g) + H2O(g)


The second step of this mechanism israte-determining (slow). What wouldthe rate law for this reaction be if thefirst step were rate-determining?



1 a) Rate = k [NO][H2]1/2
b) Rate = k[NO]2
c) Rate = k[NO]1/2 [H2]
d) Rate = k[NO]2 [H2]
e) Rate = k [NO][H2] 2 NO(g) -->N2O2(g)
N2O2(g) +H2(g) --> H2O(g) +N2O(g)
N2O(g) + H2(g) -->N2(g) + H2O(g)

1 a) Rate = k [NO][H2]1/2
b) Rate = k[NO]2
c) Rate = k[NO]1/2 [H2]
d) Rate = k[NO]2 [H2]
e) Rate = k [NO][H2] 1 a) Rate = k [NO][H2]1/2
b) Rate = k[NO]2
c) Rate = k[NO]1/2 [H2]
d) Rate = k[NO]2 [H2]
e) Rate = k [NO][H2] 1

Explanation / Answer

If The first one was the Rate determining step, the the rate law isonly based on that step. Rate = k[NO]2 (choice B; only write the reactant,coefficient acts as power)

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.