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 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 follow the principles of first-order kinetics and the Arrhenius equation to determine the amount of decomposition of compound A.

### Step 1: Understand the given data
- The decomposition of compound A is a first-order process.
- Activation energy (Ea) = 52.3 kJ/mol.
- A 10% solution of A is decomposed in 10 minutes at 10°C.
- We need to find the decomposition of a 20% solution after 20 minutes at 20°C.

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