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Question

(A) For the reaction,$2 NO_{2(g)} \longrightarrow 2 NO_{(g)} + O_{2(g)}$,the rate expression is given by: $r = -\frac{1}{2} \frac{d[NO_2]}{dt} = +\fra

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$X = NO, Y = O_2, Z = NO_2$

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(A) For the reaction,$2 NO_{2(g)} \longrightarrow 2 NO_{(g)} + O_{2(g)}$,the rate expression is given by: $r = -\frac{1}{2} \frac{d[NO_2]}{dt} = +\frac{1}{2} \frac{d[NO]}{dt} = +\frac{d[O_2]}{dt}$. $1$. Curve $Z$ represents the reactant $NO_2$ because its concentration decreases with time. $2$. Curves $X$ and $Y$ represent the products $NO$ and $O_2$ because their concentrations increase with time. $3$. From the stoichiometry,the rate of formation of $NO$ is twice the rate of formation of $O_2$ (i.e.,$\frac{d[NO]}{dt} = 2 \frac{d[O_2]}{dt}$). $4$. Therefore,the concentration of $NO$ increases faster than $O_2$,meaning curve $X$ corresponds to $NO$ and curve $Y$ corresponds to $O_2$. Thus,$X = NO, Y = O_2, Z = NO_2$.

Consider the reaction,$2 NO_{2(g)} \rightarrow 2 NO_{(g)} + O_{2(g)}$. In the figure below,identify the curves $X, Y$ and $Z$ associated with the three species in the reaction.

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