Write the rate equation for the following reactions:
$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$
$1.$ $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
$2.$ $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$
The rate of a reaction is defined as the change in concentration of reactants or products per unit time,divided by their respective stoichiometric coefficients.
For reaction $1$: $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
Rate $= -\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$
For reaction $2$: $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$
Rate $= -\frac{1}{2} \frac{d[HI]}{dt} = \frac{d[H_2]}{dt} = \frac{d[I_2]}{dt}$
For reaction $1$: $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
Rate $= -\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$
For reaction $2$: $2 HI_{(g)} \rightarrow H_{2(g)} + I_{2(g)}$
Rate $= -\frac{1}{2} \frac{d[HI]}{dt} = \frac{d[H_2]}{dt} = \frac{d[I_2]}{dt}$
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Write the following equations for the reaction $R \to P$: $(i)$ Average rate $(ii)$ Instantaneous rate.
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The reaction is:
$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$
The reaction is:
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View SolutionFor the reaction $2P + Q \to R$. If the rate of appearance of $R$ is $0.5 \ mol \ L^{-1} \ h^{-1}$,then the rate of disappearance of $P$ and $Q$ are:
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View SolutionIf the instantaneous rate of reaction is given as $-\frac{1}{a} \frac{d[A]}{dt} = -\frac{1}{b} \frac{d[B]}{dt} = \frac{1}{c} \frac{d[C]}{dt} = \frac{1}{d} \frac{d[D]}{dt}$,then the reaction is represented as:
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