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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:
- 6.93 × 10⁻² mol min⁻¹
- 6.93 × 10⁻⁴ mol min⁻¹
- 2.66 L min⁻¹ at STP
- 1.34 × 10⁻² mol min⁻¹
Correct answer: 6.93 × 10⁻⁴ mol min⁻¹
Solution
The correct option is right because, in a first-order reaction, the rate of reaction is directly proportional to the concentration of the reactant. At 0.05 M concentration of H2O2, the rate constant can be calculated from the initial data, leading to the formation rate of O2 being 6.93 × 10⁻⁴ mol min⁻¹.
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