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Consider the following reaction for $2 \mathrm{NO}_{2}(g)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2} \mathrm{F}(g) . \quad$ The expression for the rate of reaction in terms of the rate of change of partial pressure of reactant and product is/are
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rate $=-\frac{1}{2}\left[\frac{d p\left(\mathrm{NO}_{2}\right)}{d t}\right]$, rate $=\frac{1}{2}\left[\frac{d p\left(\mathrm{NO}_{2} \mathrm{F}\right)}{\mathrm{dt}}\right]$
$2 \mathrm{NO}_{2}(g)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2} \mathrm{F}(g)$
$$
\begin{aligned}
\text { Rate of reaction } &=-\frac{1}{2}\left[\frac{d p\left(\mathrm{NO}_{2}\right)}{d t}\right] \\
&=-\left[\frac{d p\left(F_{2}\right)}{d t}\right] \\
&=+\frac{1}{2}\left[\frac{d p\left(\mathrm{NO}_{2} F\right)}{d t}\right]
\end{aligned}
$$
$$
\begin{aligned}
\text { Rate of reaction } &=-\frac{1}{2}\left[\frac{d p\left(\mathrm{NO}_{2}\right)}{d t}\right] \\
&=-\left[\frac{d p\left(F_{2}\right)}{d t}\right] \\
&=+\frac{1}{2}\left[\frac{d p\left(\mathrm{NO}_{2} F\right)}{d t}\right]
\end{aligned}
$$
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