Question

what is the value of the constant for a second order reaction if the reactant concentration drops from .657 M to ,0981 M in 17 s?

Answer 1

Answer : The value of the constant for a second order reaction is,
`0.51M^(-1)s^(-1)`

Explanation :

The expression used for second order kinetics is:

`kt=(1)/([A_t])-(1)/([A_o])`

where,

k = rate constant = ?

t = time = 17s

`[A_t]` = final concentration = 0.0981 M

`[A_o]` = initial concentration = 0.657 M

Now put all the given values in the above expression, we get:

`k* 17s=(1)/(0.0981M)-(1)/(0.657M)`

`k=0.51M^(-1)s^(-1)`

Therefore, the value of the constant for a second order reaction is,
`0.51M^(-1)s^(-1)`