Decomposition of H 2 O 2 follows a first order reaction.In fifty minutes the concentration of H 2 O 2 decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of H 2 O 2 reaches

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

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H 2 O 2 a q → H 2 O a q + 1 2 O 2 g k = 1 t ln ⁡ a 0 a 1 = 1 50 ln ⁡ 0.5 0.125 = 1 50 ln ⁡ 4 min - 1 ⁡ Rate of disappearance of H 2 O 2 1 = Rate of appearance of O 2 1 2 R a t e O 2 = 1 2 × R a t e H 2 O 2 = 1 2 k H 2 O 2 = 1 2 × 1 50 × ln ⁡ 4 × 0.05 = 6.93 × 1 0 - 4 M min - 1 ⁡

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