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(C) For a first order reaction,the rate constant $k$ is given by the formula: $k = \frac{2.303}{t} \log_{10} \frac{[A]_0}{[A]_t}$.Given: $t = 2 	imes

Vedclass · Accepted Answer

$1.386 	imes 10^{-2}$

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(C) For a first order reaction,the rate constant $k$ is given by the formula: $k = \frac{2.303}{t} \log_{10} \frac{[A]_0}{[A]_t}$.Given: $t = 2 	imes 10^2 \ s$,$[A]_0 = 800 \ mol/dm^3$,$[A]_t = 50 \ mol/dm^3$.Substituting the values: $k = \frac{2.303}{2 	imes 10^2} \log_{10} \frac{800}{50}$.$k = \frac{2.303}{200} \log_{10} 16$.Since $\log_{10} 16 = \log_{10} 2^4 = 4 	imes 0.3010 = 1.204$.$k = \frac{2.303 	imes 1.204}{200} = \frac{2.7728}{200} = 1.3864 	imes 10^{-2} \ s^{-1}$.

Time $(s)$	$0$	$30$	$60$	$90$
Concentration $(mol \ L^{-1})$	$0.551$	$0.312$	$0.173$	$0.085$

In a first order reaction,the concentration of reactant decreases from $800 \ mol/dm^3$ to $50 \ mol/dm^3$ in $2 \times 10^2 \ s$. The rate constant of the reaction in $s^{-1}$ is:

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