Asecond order reaction of the type a+b> p was carried out in a solution that was initially .075 mol dm-3 in a and .03 mol dm-3 in b. after 1 hour, the concentration of a had fallen to .02 mol dm-3. a. calculate the rate constant. b. what is the half life of the reactant? answers: a. 16.2 dm3mol-hr-, 4.5e-3 dm3mol-s- b. 5.1e3s, 2.1e3 s

The rate constant of the reaction is .

is the half life of the reactant.

Explanation:

A+B → P

Integrated rate law for second order kinetics is given by:

A = concentration left after time t =

= Initial concentration =

t = 1 hour = 3600 seconds

Half life for second order kinetics is given by:

The rate constant of the reaction is .

is the half life of the reactant.