Question

The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If the rate constant is 2.50 × 10−4 s−1, what is the half-life of this reaction?

Answer 1

Answer:

2,772 seconds is the half-life of this reaction.

Explanation:

$2N_2O_5(g)\rightarrow 4NO_2(g) + O_2(g)$

The rate constant of the reaction = k = $2.50\times 10^{-4} s^{-1}$

From the unit of rate constant, the order of reaction will be 1.This is because the unit of the rate constant the reaction following first order kinetics is time inverse.

For first order kinetic half life ($t_{1/2}$) and rate constant (k)are related by :

$t_{1/2}=\frac{0.693}{k}$

$t_{1/2}=\frac{0.693}{2.50\times 10^{-4} s^{-1}}=2,772 s$

2,772 seconds is the half-life of this reaction.