Which of the following values would you expect for the ratio of half-lives for a reaction with starting concentrations of 0.05m and 0.01m, t1/2 (0.05m) / t1/2 (0.01m), if a reaction is known to be first order?

The ratio of half-lives for a reaction with starting concentrations of 0.05M and 0.01M, t1/2 (0.05M) / t1/2 (0.01M) = 1, if a reaction is known to be first order.

Explanation:

the half-life of the reaction is constant and does not depend on the value of the initial concentration.

half-life (t1/2) = 0.693/k,

where, k is the rate constant of the reaction.

So, half;life of first-order reaction is constant whatever the initial concentration.

So the ratio of t1/2 (0.05M) / t1/2 (0.01M) = 1

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