A certain second-order reaction (B→products) has a rate constant of 1.30×10−3 M−1⋅s−1 at 27 ∘C and an initial half-life of 224 s . What is the concentration of the reactant B after one half-life?

Explanation:

By definition one half-life is the time to reduce the initial concentration to half.

For a second order reaction the rate law equations are:

The half-life equation is:

Thus, substitute the rate constant   and the half-life time 224s to find [A]₀:

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .