Problem PageQuestionConsider the following elementary reaction:2NO2(g) →NO3(g) +NO(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 NO3 in terms of k1, k−1, and the equilibrium concentrations of NO2 and NO.
Question
Problem PageQuestionConsider the following elementary reaction:2NO2(g) →NO3(g) +NO(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 NO3 in terms of k1, k−1, and the equilibrium concentrations of NO2 and NO.
Solution
The equilibrium constant (K) for a reaction is given by the ratio of the rate constants for the forward and reverse reactions. In this case, K = k1/k−1.
At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. Therefore, we can write the following expressions for the rates of the forward and reverse reactions:
Rate of forward reaction = k1 * [NO2]^2 Rate of reverse reaction = k−1 * [NO3] * [NO]
Setting these equal to each other gives:
k1 * [NO2]^2 = k−1 * [NO3] * [NO]
We can rearrange this to solve for [NO3]:
[NO3] = (k1/k−1) * [NO2]^2 / [NO]
But since K = k1/k−1, we can substitute K into the equation to get:
[NO3] = K * [NO2]^2 / [NO]
This is the expression for the equilibrium concentration of NO3 in terms of K, [NO2], and [NO].
Similar Questions
Consider the following elementary reaction:N2O(g) →N2(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 O in terms of k1, k−1, and the equilibrium concentrations of N2O and N2.=O
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
Given the equilibrium constant (K) which side of the reaction is favoured N2(g) + 3H2(g) 2NH3(g) Keq = 735
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.