`O_(2)` is evolved by heating `KClO_(3)` using `MnO_(2)` as a catalyst
`2KClO_(3) overset(MnO_(2))to 2KCl+3O_(2)`
Calculate the mass of `KClO_(3)` required to produce 6.72 litre of `O_(2)` at S.T.P. [atomic masses of K = 39, Cl = 35.5, O = 16).

Explanation

To solve the problem of calculating the mass of \( KClO_3 \) required to produce 6.72 liters of \( O_2 \) at STP, we can follow these steps:

### Step 1: Write the balanced chemical equation.
The balanced equation for the decomposition of potassium chlorate (\( KClO_3 \)) is:
\[ 2 KClO_3 \xrightarrow{MnO_2} 2 KCl + 3 O_2 \]

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