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From the following data find the order of decomposition of $H_{2} O_{2}$ in aqueous solution.
Time (in minutes) 0 10 20
Volume(in c.c. of $K M n O_{4}$ ) 22.8 13.3 8.25

If X is order, then X is ____.

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Solution

From the given, data, it can be concluded that the reaction is of the first order.

For first order reaction, $k = \frac{2.303}{t} l o g \frac{a}{a - x}$

For $t = 10$ , $k = \frac{2.303}{10} l o g \frac{22.8}{13.3} = 0.05$

For $t = 20$ , $k = \frac{2.303}{20} l o g \frac{22.8}{8.23} = 0.05$

Thus, $X = 1$

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