Consider the following reaction: $2 NO_{2(g)} + F_{2(g)} \longrightarrow 2 NO_2F_{(g)}$. The expression for the rate of reaction in terms of the rate of change of partial pressure of reactant and product is/are:
- Arate $= -\frac{1}{2} \left[ \frac{dp(NO_2)}{dt} \right]$
- Brate $= \frac{1}{2} \left[ \frac{dp(NO_2)}{dt} \right]$
- Crate $= -\frac{1}{2} \left[ \frac{dp(NO_2F)}{dt} \right]$
- Drate $= \frac{1}{2} \left[ \frac{dp(NO_2F)}{dt} \right]$
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Why does the rate of reaction increase with respect to product?
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View Solution$5 Br^{-}_{(aq)} + BrO^{-}_{3(aq)} + 6 H^{+}_{(aq)} \rightarrow 3 Br_{2(aq)} + 3 H_{2}O_{(l)}$
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