Suppose the reduction of nitric oxide proceeds by the following mechanism: H_2(g

Question

Suppose the reduction of nitric oxide proceeds by the following mechanism: H_2(g) + 2NO(g) rightarrow N_2O(g) + H_2O(g) H_2(g) + N_2O(g) rightarrow N_2(g) + H_2O(g) Suppose also k_1>>k_2. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. Express the rate constant k for the overall chemical reaction in terms of k_1, k_2, and (if necessary) the rate constants k_-1 and k_-2 for the reverse of the two elementary reactions in the mechanism.

Explanation / Answer

Balanced chemical equation

H2 + 2NO = N2O + H2O

H2 + N2O = N2 + H2O

add

H2 + 2NO + H2 + N2O= N2O + H2O+ N2 + H2O

cancel common terms

2H2 + 2NO = H2O + N2 + H2O

experimentally observable rate law...

we only care about the SLWOEST step, since that will model accurately the rate

so choose K2, since it is the slowest rate

for K:

K = K1*K2 since both are forward directions

Related Questions

Navigate

• Browse (All)
• Browse S
• Subjects

---

---

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