Decomposition of

Question:

Decomposition of $\mathrm{H}_{2} \mathrm{O}_{2}$ follows a first order reaction. In fifty minutes the concentration of $\mathrm{H}_{2} \mathrm{O}_{2}$ decreases from $0.5$ to $0.125 \mathrm{M}$ in one such decomposition. When the concentration of $\mathrm{H}_{2} \mathrm{O}_{2}$ reaches $0.05 \mathrm{M}$, the rate of formation of $\mathrm{O}_{2}$ will be :-

  1. $1.34 \times 10^{-2} \mathrm{~mol} \mathrm{~min}{ }^{-1}$

  2. $6.93 \times 10^{-2} \mathrm{~mol} \mathrm{~min}{ }^{-1}$

  3. $6.93 \times 10^{-4} \mathrm{~mol} \mathrm{~min}{ }^{-1}$

  4. $2.66 \mathrm{~L} \mathrm{~min}^{-1}$ at STP

Correct Option: , 3

Solution:

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