Problem PageQuestionConsider the following elementary reaction:NO(g) +O2(g) →NO2(g) +O(g)Suppose we let k1 stand for the rate constant of this reaction, and k−1 stand for the rate constant of the reverse reaction.Write an expression that gives the equilibrium concentration of NO in terms of k1, k−1, and the equilibrium concentrations of O2, NO2, and O
Question
Problem PageQuestionConsider the following elementary reaction:NO(g) +O2(g) →NO2(g) +O(g)Suppose we let k1 stand for the rate constant of this reaction, and k−1 stand for the rate constant of the reverse reaction.Write an expression that gives the equilibrium concentration of NO in terms of k1, k−1, and the equilibrium concentrations of O2, NO2, and O
Solution
The rate of the forward reaction can be expressed as: Rate1 = k1[NO][O2]
The rate of the reverse reaction can be expressed as: Rate-1 = k-1[NO2][O]
At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. Therefore, we can set Rate1 equal to Rate-1 and solve for [NO]:
k1[NO][O2] = k-1[NO2][O]
Rearranging to solve for [NO] gives:
[NO] = (k-1/k1) * ([NO2][O]/[O2])
Similar Questions
Write the rate law for the following elementary reaction:2NO(g) + O2(g) → 2NO2(g)Use k1 to stand for the rate constant.
Which of the following is the equilibrium constant expression for the reaction?2NO(g) + O2(g) → 2NO2(g)
The equilibrium constant, KC, for the following reaction is 2.5 × 10-3N2(g) + O2(g) ⇌ 2NO(g)If [N2]eq = 0.75 M and [NO]eq = 0.090, then [O2]eq
Write the rate law for the following elementary reaction:O 3 (g) + NO(g) → O 2 (g) + NO 2 (g)
How can you determine the rate law of the following reaction?2NO (g) + O2 (g) → 2NO2 (g)
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.