Find the rate of the following reaction: 2 N | vedclass

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Question

(A) The rate of reaction is given by the expression: $	ext{Rate} = -\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}

Vedclass · Accepted Answer

$1.3 	imes 10^{-5} \ mol \ dm^{-3} \ s^{-1}$

Vedclass · Answer

(A) The rate of reaction is given by the expression: $	ext{Rate} = -\frac{1}{2} \frac{d[N_2O_5]}{dt} = \frac{1}{4} \frac{d[NO_2]}{dt} = \frac{d[O_2]}{dt}$.Given that the concentration of $NO_2$ increases by $\Delta[NO_2] = 5.2 	imes 10^{-3} \ M$ in $\Delta t = 100 \ s$.The rate of formation of $NO_2$ is $\frac{d[NO_2]}{dt} = \frac{5.2 	imes 10^{-3} \ M}{100 \ s} = 5.2 	imes 10^{-5} \ M \ s^{-1}$.Therefore,the rate of the reaction is $	ext{Rate} = \frac{1}{4} 	imes (5.2 	imes 10^{-5} \ M \ s^{-1}) = 1.3 	imes 10^{-5} \ mol \ dm^{-3} \ s^{-1}$.

Find the rate of the following reaction: $2 \ N_2O_{5(g)} \rightarrow 4 \ NO_{2(g)} + O_{2(g)}$ if the concentration of $NO_2$ increases to $5.2 \times 10^{-3} \ M$ in $100 \ s$.

Similar Questions

Observe the following reaction: $2 A + B \longrightarrow C$. The rate of formation of $C$ is $2.2 \times 10^{-3} \ mol \ L^{-1} \ min^{-1}$. What is the value of $-\frac{d[A]}{d t}$ (in $mol \ L^{-1} \ min^{-1}$)?

$5 Br^{-}_{(aq)} + BrO^{-}_{3(aq)} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2(aq)} + 3 H_{2}O_{(l)}$
The rate of consumption of $H^{+}$ is $x \ mol \ L^{-1} \ s^{-1}$.
$(a)$ What is the rate of consumption of $Br^{-}$?
$(b)$ What is the rate of formation of $Br_{2}$?

For the reaction $2A + 3B \rightarrow 4C$,the rate of reaction is expressed as:

For the reaction $2A + B \rightarrow 3C + D$,which of the following options does not represent the correct rate of the reaction?

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