Question

The rate law for the reaction described by the equation
2 N2O (g) ----> 2 N2 (g) + O2 (g)
is second order in N2O (g). The reaction was carried out at 900 K with an initial concentration of N2O (g) of 3.5 × 10^–2 M. If it took 91.3 minutes for [N2O] to fall to half it original value, what is the value of the rate constant for this reaction?

A) 3.5 × 10^–3 M^-1 * s^-1

B) 4.8 × 10^–3 M^-1 * s^-1

C) 5.2 × 10^–3 M^-1 * s^-1

D) 8.4 × 10^–3 M^-1 * s^-1

Answer 1