The rate constant,k,of a zero order reaction | vedclass

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(C) For a zero order reaction,the rate of reaction is equal to the rate constant,$k$.$r = k = y 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}$.From the stoic

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$3 y 	imes 10^{-4}$

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(C) For a zero order reaction,the rate of reaction is equal to the rate constant,$k$.$r = k = y 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}$.From the stoichiometry of the reaction $2 NH_3(g) ightarrow N_2(g) + 3 H_2(g)$,the rate of reaction is given by:$r = -\frac{1}{2} \frac{d[NH_3]}{dt} = \frac{d[N_2]}{dt} = \frac{1}{3} \frac{d[H_2]}{dt}$.Therefore,the rate of formation of hydrogen is:$\frac{d[H_2]}{dt} = 3 	imes r = 3 	imes (y 	imes 10^{-4}) = 3 y 	imes 10^{-4} \ mol \ L^{-1} \ s^{-1}$.

The rate constant,$k$,of a zero order reaction $2 NH_3(g) \xrightarrow[1130 \ K]{Pt} N_2(g) + 3 H_2(g)$ is $y \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$. The rate of formation of hydrogen (in $mol \ L^{-1} \ s^{-1}$) is

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