Question

The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42 x 10-4 s-1 at a certain temperature. How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration

Answer 1

Answer: The time taken is 9764.4 seconds

Step-by-step explanation:

Rate law expression for first order kinetics is given by the equation:

`k=(2.303)/(t)\log([A_o])/([A])`

where,

k = rate constant =
`1.42* 10^(-4)s^(-1)`

t = time taken for decay process = ? sec

`[A_o]` = initial amount of the reactant = 100 grams

[A] = amount left after decay process = 25 grams

Putting values in above equation, we get:

`1.42* 10^(-4)=(2.303)/(t)\log(100)/(25)\\\\t=9764.4s`

Hence, the time taken is 9764.4 seconds