At a certain temperature the rate of this reaction is second order in nh4oh with a rate constant of 34.1 m^-1*s^-1:
nh4oh(aq) > nh3(aq) + h2o (aq)
suppose a vessel contains nh4oh at a concentration of 0.100m. calculate how long it takes for the concentration of nh4oh to decrease to 0.0240 m. you may assume no other reaction is important. round your answer to 2 significant digits.

It will take 0.93 seconds the concentration of to decrease to 0.0240 M.

Explanation:

Integrated rate law for second order kinetics is given by:

k = rate constant

= half life of reaction

= initial concentration

a= concentration left after time t

We have :

Initial concentration of ammonium hydroxide =

Final concentration of ammonium hydroxide after time t=

Rate constant of the reaction = k =

Solving for t:

t = 0.93 seconds

It will take 0.93 seconds the concentration of to decrease to 0.0240 M.

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