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 reache

Question

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 → H 2 O + 1 2 O 2 - d [ H 2 O 2 ] dt = d [ H 2 O ] dt = 2 d [ O 2 ] dt t 1 2 = 25 t 1 2 = 0 .69314 k k = 0 .69314 25 rate of reaction = k [ H 2 O 2 ] ∴ d [ O 2 ] dt = 1 2 × k [ H 2 O 2 ] = 1 2 × 0.69314 25 × 0.05 = 6.93 × 10 - 4 m o l m i n - 1

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