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.

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error