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Decomposition of {H}_{{{2}}}{O}_{{{2}}} follows a first order

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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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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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Question Text	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 :
Answer Type	Video solution: 1
Upvotes	150