Nitric oxide reacts with H_2 according to the | vedclass

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(B) 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

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

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(B) 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 $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$,the rate expression is: Rate $= -\frac{1}{2} \frac{d[NO]}{dt} = -\frac{1}{2} \frac{d[H_2]}{dt} = \frac{d[N_2]}{dt} = \frac{1}{2} \frac{d[H_2O]}{dt}$ Comparing the terms for $N_2$ and $H_2O$: $\frac{d[N_2]}{dt} = \frac{1}{2} \frac{d[H_2O]}{dt}$ This implies $\frac{d[H_2O]}{dt} = 2 \frac{d[N_2]}{dt}$. Comparing the terms for $N_2$ and $H_2$: $\frac{d[N_2]}{dt} = -\frac{1}{2} \frac{d[H_2]}{dt}$. Thus,option $B$ is the correct relationship.

Time $(s)$	$0$	$100$	$200$	$300$	$400$	$700$	$800$
$[C_4H_9Cl]$ $(mol \, L^{-1})$	$0.100$	$0.082$	$0.067$	$0.055$	$0.044$	$0.021$	$0.017$

Nitric oxide reacts with $H_2$ according to the reaction:
$2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$
Identify the correct relationship for the rate of consumption of reactants and the rate of formation of products.

Similar Questions

For the reaction $N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}$,the reaction occurs under specific temperature and partial pressure conditions. The rate of formation of $NH_3$ is $0.001 \, kg \, h^{-1}$. The rate of consumption of $H_2$ under the same conditions is ...... $kg \, h^{-1}$.

What is the rate of disappearance of $B$ in the following reaction? $2A + B \rightarrow 3C$,if the rate of appearance of $C$ is $1.3 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$.

For the reaction,$A + B \to 2C + D$,which one is the incorrect statement?

Which of the following is a correct representation of the reaction rate for the reaction stated below?
$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

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Nitric oxide reacts with $H_2$ according to the reaction: $2 NO_{(g)} + 2 H_{2(g)} \rightarrow N_{2(g)} + 2 H_{2}O_{(g)}$Identify the correct relationship for the rate of consumption of reactants and the rate of formation of products.