Find the average rate of formation $\mathrm{O}_{2(\mathrm{~g})}$ in the following reaction. $\begin{aligned}…

Find the average rate of formation $\mathrm{O}_{2(\mathrm{~g})}$ in the following reaction. $\begin{aligned} & 2 \mathrm{NO}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \\ & {\left[-\frac{\Delta[\mathrm{NO}]}{\Delta \mathrm{t}}\right]=\mathrm{x} \mathrm{moldm}^{-3} \mathrm{~s}^{-1}} \end{aligned}$
  1. $\frac{x}{2} \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}$
  2. $\mathrm{x} \mathrm{mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}$
  3. $2 \times \mathrm{mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}$
  4. $4 \times \mathrm{mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}$

Solution

Average rate of reaction $=-\frac{1}{2} \frac{\Delta\left[\mathrm{NO}_2\right]}{\Delta \mathrm{t}}=\frac{1}{2} \frac{\Delta\left[\mathrm{NO}_2\right]}{\Delta \mathrm{t}}=\frac{\Delta\left[\mathrm{O}_2\right]}{\Delta \mathrm{t}}$ Rate of formation of $\mathrm{O}_2=\frac{\Delta\left[\mathrm{O}_2\right]}{\Delta \mathrm{t}}$ $\begin{aligned} & =\frac{1}{2} \frac{-\Delta\left[\mathrm{NO}_2\right]}{\Delta \mathrm{t}} \\ & =\frac{1}{2} \times \mathrm{x}=\frac{\mathrm{x}}{2} \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1} \end{aligned}$

Asked in: MHT CET 2023 (09 May Shift 2)

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