In a reaction N_{2(g)} + 3H_{2(g)} to 2NH_{3( | vedclass

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(C) For the reaction $N_{2(g)} + 3H_{2(g)} 	o 2NH_{3(g)}$,the rate expression is given by:Rate $= -\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt}

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$1.25 	imes 10^{-4}, 3.75 	imes 10^{-4}$

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(C) For the reaction $N_{2(g)} + 3H_{2(g)} 	o 2NH_{3(g)}$,the rate expression is given by:Rate $= -\frac{d[N_2]}{dt} = -\frac{1}{3} \frac{d[H_2]}{dt} = \frac{1}{2} \frac{d[NH_3]}{dt}$Given,rate of appearance of $NH_3$ is $\frac{d[NH_3]}{dt} = 2.5 	imes 10^{-4} \, mol \, L^{-1} \, s^{-1}$.Rate of reaction $= \frac{1}{2} 	imes \frac{d[NH_3]}{dt} = \frac{1}{2} 	imes 2.5 	imes 10^{-4} = 1.25 	imes 10^{-4} \, mol \, L^{-1} \, s^{-1}$.Rate of disappearance of $H_2$ is $-\frac{d[H_2]}{dt}$.From the rate expression,$-\frac{d[H_2]}{dt} = \frac{3}{2} \frac{d[NH_3]}{dt} = \frac{3}{2} 	imes 2.5 	imes 10^{-4} = 3.75 	imes 10^{-4} \, mol \, L^{-1} \, s^{-1}$.

In a reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$,the rate of appearance of $NH_3$ is $2.5 \times 10^{-4} \, mol \, L^{-1} \, s^{-1}$. The rate of reaction and rate of disappearance of $H_2$ will be (in $mol \, L^{-1} \, s^{-1}$):

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