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Decomposition of H2O2 follows a first order reaction. In fifty minutes the concentration of H2O2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H2O2 reaches 0.05 M, the rate of formation of O2 will be:
- 2.66 L min−1 at STP
- 1.34 × 10−2 mol min−1
- 6.96 × 10−2 mol min−1
- 6.93 × 10−4 mol min−1
Correct answer: 6.93 × 10−4 mol min−1
Solution
The correct option is derived from the first-order kinetics of the decomposition reaction, where the rate of reaction is proportional to the concentration of H2O2. At 0.05 M concentration, the calculated rate of formation of O2, based on the stoichiometry of the reaction and the rate constant, results in 6.93 × 10−4 mol min−1.
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