Question

At a certain temperature the rate of this reaction is second order in with a rate constant of Suppose a vessel contains at a concentration of . Calculate how long it takes for the concentration of to decrease to . You may assume no other reaction is important. Round your answer to significant digits.

Answer 1

Answer: The given question is incomplete. The complete question is:

At a certain temperature the rate of this reaction is second order in
`NH_4OH` with a rate constant of
`34.1M^(-1)s^(-1)` .
`NH_4OH(aq)\rightarrow NH_3(aq)+H_2O(aq)`

Suppose a vessel contains
`NH_4OH` at a concentration of 0.100 M Calculate how long it takes for the concentration of
`NH_4OH` to decrease to 0.0240 M. You may assume no other reaction is important. Round your answer to 2 significant digits.

Answer: It takes 0.93 seconds for the concentration
`NH_4OH` to decrease to 0.0240 M.

Step-by-step explanation:

Integrated rate law for second order kinetics is given by:

`(1)/(a)=kt+(1)/(a_0)`

`a_0` = initial concentration = 0.100 M

a= concentration left after time t = 0.0240 M

k = rate constant =
`34.1M^(-1)s^(-1)`

t = time taken for decomposition = ?

`(1)/(0.0240)=34.1* t+(1)/(0.100)`

`t=0.93s`

Thus it takes 0.93 seconds for the concentration
`NH_4OH` to decrease to 0.0240 M.