The decompoistion of compound `A` in solution is a first order process with an activation energy of `52.3 kJ mol^(-1)`. A `10%` solution of `A` is `10%` decomposed in `10 min` at `10^(@)C`. How much decompoistion would be observed with a `20%` solution after `20 min` at `20^(@)C`.

Explanation

To solve the problem step by step, we will use the first-order kinetics equation and the Arrhenius equation to find the decomposition of compound A under the given conditions.

### Step 1: Determine the rate constant (k) at 10°C

Given that a 10% solution of A is 10% decomposed in 10 minutes at 10°C, we can use the first-order kinetics formula:

\[
k = \frac{2.303}{t} \log \left( \frac{[A_0]}{[A]} \right)
...