(B) The rate law for the first-order reaction is $r = k[H_2O_2]$.Given: $k = 3 \times 10^{-3} \ min^{-1} = \frac{3 \times 10^{-3}}{60} \ s^{-1} = 5 \t

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(B) The rate law for the first-order reaction is $r = k[H_2O_2]$.Given: $k = 3 \times 10^{-3} \ min^{-1} = \frac{3 \times 10^{-3}}{60} \ s^{-1} = 5 \times 10^{-5} \ s^{-1}$.Given: $r = 2 \times 10^{-4} \ M \ s^{-1}$.Substituting the values in the rate law: $2 \times 10^{-4} = (5 \times 10^{-5}) \times [H_2O_2]$.$[H_2O_2] = \frac{2 \times 10^{-4}}{5 \times 10^{-5}} = \frac{20 \times 10^{-5}}{5 \times 10^{-5}} = 4 \ M$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

A
$6.67 \times 10^{-3} \ M$
B
$4 \ M$
C
$0.08 \ M$
D
$2 \ M$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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The rate constant of the reaction,$2 H_2O_2 \rightarrow 2 H_2O + O_2$ is $3 \times 10^{-3} \ min^{-1}$. At what concentration of $H_2O_2$ will the rate of reaction be $2 \times 10^{-4} \ M \ s^{-1}$?

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What will be the unit of the rate constant for the following reaction?
$C_2H_{4(g)} + H_{2(g)} \rightarrow C_2H_{6(g)}$