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.

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