Question

In the reaction 2\(\mathrm{N_2O_5(g)} \rightarrow 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}, \)the rate of formation of\( \mathrm{NO_2(g)} and \mathrm{O_2(g)} \) are in the ratio

• A. \(1:4\)
• B. \(1:1\)
• C. \(6:1\)
• D. \(4:1\)

Hint:

Rates of formation of products are directly proportional to their stoichiometric coefficients in the balanced equation.

Answer 1

The Correct Option is A

Step 1: Use stoichiometric coefficients.
From the balanced chemical equation:
\[ 2\mathrm{N_2O_5} \rightarrow 4\mathrm{NO_2} + \mathrm{O_2} \]
Step 2: Relate rate of formation to coefficients.
The rate of formation of products is proportional to their stoichiometric coefficients.
Thus, the rate of formation of \(\mathrm{NO_2}\) and \(\mathrm{O_2}\) is in the ratio \(4:1\).
Step 3: Express as asked ratio.
The ratio of rate of formation of \(\mathrm{O_2}\) to \(\mathrm{NO_2}\) is \(1:4\).
Step 4: Conclusion.
Hence, the required ratio is \(1:4\).