Decomposition of `H_(2)O_(2)` is a first-order reaction. A solution of `H_(2)O_(2)` labelled as `20` volumes was left open. Due to this some `H_(2)O_(2)` decomposed. To determine the new volume strength after `6` hours, `10 mL` of this solution was diluted to `100 mL`. `10 mL` of this diluted solution was titrated against `25 mL `of `0.025 m KMnO_(4)` acidified solution. Calculate the rate constant for decomposition of `H_(2)O_(2)`.

Decomposition of `H_(2)O_(2)` is a first-order reaction. A solution of

1.	Decomposition of `H_(2)O_(2)` is a first-order reaction. A solution of `H_(2)O_(2)` labelled as `20` volumes was left open. Due to this some `H_(2)O_(2)` decomposed. To determine the new volume strength after `6` hours, `10 mL` of this solution was diluted to `100 mL`. `10 mL` of this diluted solution was titrated against `25 mL `of `0.025 m KMnO_(4)` acidified solution. Calculate the rate constant for decomposition of `H_(2)O_(2)`.
Answer» Correct Answer - `0.022 hr^(-1);`

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