The reaction 2A rightarrow 2B + C has a rate | vedclass

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(C) The unit of the rate constant $k$ is $s^{-1}$,which indicates that the reaction is a $1^{st}$ order reaction.For a $1^{st}$ order reaction,the int

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Plot of $\ln [A]$ vs $t$ will be a straight line

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(C) The unit of the rate constant $k$ is $s^{-1}$,which indicates that the reaction is a $1^{st}$ order reaction.For a $1^{st}$ order reaction,the integrated rate equation is given by $\ln [A] = \ln [A]_0 - kt$.Comparing this with the equation of a straight line $y = mx + c$,where $y = \ln [A]$,$x = t$,$m = -k$ (slope),and $c = \ln [A]_0$ (intercept).Therefore,a plot of $\ln [A]$ versus $t$ will be a straight line with a negative slope equal to $-k$.

The reaction $2A \rightarrow 2B + C$ has a rate constant of $1.2 \times 10^{-2} \ s^{-1}$. Which of the following is correct?

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