Now consider the decomposition of dinitrogen monoxide. N2O(g) → N2(g) + ½ O2(g) rate = k[N2O]2 Starting with an initial concentration of 1.0 M, what is the half-life of the reaction?

The Half life is equal to the inverse of the rate constant (1/k).

Explanation:

The half life of any reaction is the amount of time it takes to consume half of the starting material.

For a second-order reaction, the half-life is inversely related to the initial concentration of the reactant (A).

It is mathematically given as;

t1/2 = 1 / k[A]o

where;

t1/2 = Half life

k = Rate constant

[A]o = Initial Concentration

Since the initial concentration is 1.0 M;

Half life = 1 / k(1) = 1 / k

The Half life is equal to the inverse of the rate constant.

the answer is definitely c.

the answer is 0.42 is that is an option. this question provides no info