The reaction A_{(g)} to 2B_{(g)} + C_{(g)} ob | vedclass

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(D) The given reaction is a first-order reaction as the rate law is $r = K[A]$.For a first-order reaction,the integrated rate equation is: $\ln \frac{

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$0.79$

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(D) The given reaction is a first-order reaction as the rate law is $r = K[A]$.For a first-order reaction,the integrated rate equation is: $\ln \frac{[A]_0}{[A]_t} = Kt$ or $\ln \frac{n_0}{n_t} = Kt$.Given: $K = 0.023 \ s^{-1}$,$t = 50 \ s$,$n_0 = 2.5 \ moles$.Substituting the values: $\ln \frac{2.5}{n_t} = 0.023 	imes 50$.$\ln \frac{2.5}{n_t} = 1.15$.Taking the exponential of both sides: $\frac{2.5}{n_t} = e^{1.15} \approx 3.158$.$n_t = \frac{2.5}{3.158} \approx 0.79 \ moles$.

The reaction $A_{(g)} \to 2B_{(g)} + C_{(g)}$ obeys the rate law,$r = K[A]$ where $K = 0.023 \ s^{-1}$. If $2.5 \ moles$ of $A$ were taken in a $5 \ L$ flask,how many moles of $A$ would remain left after $50 \ seconds$?

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