`18.625g KCl` is formed due to decomposition of `KClO_(4)` in reaction
`KClO_(4)(s)rarr KCl(s)+2O_(2)(g)`
Find volume of `O_(2)` obtained at `STP`[Atomic mass `K = 39 Cl = 35.5]`

Explanation

To solve the problem step by step, we will follow these instructions:

### Step 1: Write the balanced chemical equation
The decomposition of potassium perchlorate (KClO₄) can be represented as:
\[ \text{KClO}_4(s) \rightarrow \text{KCl}(s) + 2 \text{O}_2(g) \]

### Step 2: Calculate the molar mass of KCl
The molar mass of KCl can be calculated using the atomic masses provided:
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