The reaction of NO and O₂ produces NO₂.
2 NO(g) + O₂(g) $\to$ 2 NO₂(g)
The reaction is second-order with respect to NO(g) and first-order with respect to O₂(g) .At a given temperature,the rate constant,k,equals 4.7 $\times$ 10² M^-2s^-1.What is the rate of reaction when the initial concentrations of NO and O₂ are 0.025 M and 0.015 M,respectively?

Question

The reaction of NO and O₂ produces NO₂.
2 NO(g) + O₂(g)

\to

2 NO₂(g)
The reaction is second-order with respect to NO(g) and first-order with respect to O₂(g) .At a given temperature,the rate constant,k,equals 4.7

\times

10² M^-2s^-1.What is the rate of reaction when the initial concentrations of NO and O₂ are 0.025 M and 0.015 M,respectively?

Quizplus · Accepted Answer

The rate law for the reaction is given by:

Rate = k[NO]^2[O2]

Substituting the given values:

Rate = (4.7 x 10^-10 M^-2s^-1) x (0.025 M)^2 x (0.015 M) = 4.4 x 10^-13 M/s = 4.4 x 10^-10 mol/L/s

Therefore, the correct choice is B, 4.4 x 10^-10 M/s.

The Reaction of NO and O2 Produces NO2 →\to→ 2 NO2(g) the Reaction Is Second-Order with Respect to NO(g)and

The Reaction of NO and O₂ Produces NO₂ $\to$ 2 NO₂(g)
the Reaction Is Second-Order with Respect to NO(g)and