At 27,^oC,for the reaction,N_2O_{4(g)} to 2NO | vedclass

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(B) The rate of reaction in terms of pressure is given as $Rate_p = 6 	imes 10^{-3} \, atm \, min^{-1}$.Using the ideal gas equation $PV = nRT$,we ha

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$2.4 	imes 10^{-4}$

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(B) The rate of reaction in terms of pressure is given as $Rate_p = 6 	imes 10^{-3} \, atm \, min^{-1}$.Using the ideal gas equation $PV = nRT$,we have $P = (n/V)RT = CRT$,where $C$ is the concentration in $mol \, L^{-1}$.Therefore,the rate in terms of concentration is $Rate_c = \frac{Rate_p}{RT}$.Given $T = 27 + 273 = 300 \, K$ and $R = 0.0821 \, L \, atm \, K^{-1} \, mol^{-1}$.$Rate_c = \frac{6 	imes 10^{-3}}{0.0821 	imes 300} = \frac{6 	imes 10^{-3}}{24.63} \approx 2.436 	imes 10^{-4} \, mol \, L^{-1} \, min^{-1}$.Rounding to the nearest option,the value is $2.4 	imes 10^{-4} \, mol \, L^{-1} \, min^{-1}$.

At $27\,^oC$,for the reaction,$N_2O_{4(g)} \to 2NO_{2(g)}$,the rate of reaction is $6 \times 10^{-3} \, atm \, min^{-1}$. Find the rate of the same reaction in terms of $mol \, L^{-1} \, min^{-1}$.

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