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Question

(C) The reaction is a first order reaction. Since the concentration decreases from $0.2 \ M$ to $0.1 \ M$ (which is half of the initial concentration)

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$6.93 	imes 10^{-3} \ min^{-1}$

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(C) The reaction is a first order reaction. Since the concentration decreases from $0.2 \ M$ to $0.1 \ M$ (which is half of the initial concentration),the time taken is the half-life period,$t_{1/2} = 100 \ minutes$. For a first order reaction,the rate constant $k$ is given by the formula: $k = \frac{0.693}{t_{1/2}}$. Substituting the value: $k = \frac{0.693}{100 \ min} = 6.93 	imes 10^{-3} \ min^{-1}$.

For a first order reaction,the concentration of reactant decreases from $0.2 \ M$ to $0.1 \ M$ in $100 \ minutes$. What is the rate constant of the reaction?

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