Consider the following elementary reaction: NO2(g) + O3(g) → NO3(g) +

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Consider the following elementary reaction: NO2(g) + O3(g) → NO3(g) + O2(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 O2 in terms of k1, k−1, and the equilibrium concentrations of NO2, O3, and NO3. [O2] =

Consider the following elementary reaction: NO2(g) + O3(g) → NO3(g) + O2(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 O2 in terms of k1, k−1, and the equilibrium concentrations of NO2, O3, and NO3. [O2] =

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Consider the following elementary reaction:

{N O}_{2} (g) + O_{3} (g) \to {N O}_{3} (g) + O_{2} (g)

Suppose we let

k_{1}

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_{2}

in terms of

k_{1}, k_{- 1}

, and the equilibrium concentrations of

{N O}_{2}, O_{3}

, and

{N O}_{3}

.

[O_{2}] =

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