The reaction 2a → a2 was experimentally determined to be second order with a rate constant, k, equal to 0.0265 m–1min–1. if the initial concentration of a was 4.00 m, what was the concentration of a (in m) after 180.0 min?

0.2 M

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

Integrated rate law for second order kinetics is given by:

t= time taken for the reaction = 180 min

k = rate constant =

= initial concentration = 4 M

a= concentration left after time t = ?

Putting in the values we get:

Thus the concentration of A after 180.0 min is 0.2M

helium

oxygen

neon

sodium