For the chemical reaction: N_{2(g)} + 3H_{2(g | vedclass

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Question

(A) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a}\frac{d[A]}{dt} = -\frac{1}{b}\frac{d[B

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Rate $= -\frac{d[N_2]}{dt} = -\frac{1}{3}\frac{d[H_2]}{dt} = \frac{1}{2}\frac{d[NH_3]}{dt}$

Vedclass · Answer

(A) For a general reaction $aA + bB \rightarrow cC + dD$,the rate of reaction is given by: Rate $= -\frac{1}{a}\frac{d[A]}{dt} = -\frac{1}{b}\frac{d[B]}{dt} = \frac{1}{c}\frac{d[C]}{dt} = \frac{1}{d}\frac{d[D]}{dt}$. For the given reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the stoichiometric coefficients are $a=1$,$b=3$,and $c=2$. Substituting these values,we get: Rate $= -\frac{d[N_2]}{dt} = -\frac{1}{3}\frac{d[H_2]}{dt} = \frac{1}{2}\frac{d[NH_3]}{dt}$.

For the chemical reaction: $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the rate of reaction can be expressed in terms of the concentration of $N_{2(g)}$,$H_{2(g)}$,or $NH_{3(g)}$ with respect to time. Identify the correct relationship between these rates.

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