Two moles of N2 O4 is heated to form NO and O2. As soon as NO and O2 are formed they react to fo

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Two moles of N2 O4 is heated to form NO and O2. As soon as...

Two moles of $\mathrm{N}_2 \mathrm{O}_4$ is heated to form NO and $\mathrm{O}_2$. As soon as NO and $\mathrm{O}_2$ are formed they react to form $\mathrm{N}_2 \mathrm{O}_5$. Two equilibria $$ \begin{aligned} \mathrm{N}_2 \mathrm{O}_4 & \rightleftharpoons 2 \mathrm{NO}+\mathrm{O}_2 \\ 2 \mathrm{NO}+\frac{3}{2} \mathrm{O}_2 & \rightleftharpoons \mathrm{~N}_2 \mathrm{O}_5 \end{aligned} $$ Are simultaneously established. At equilibrium, the degree of dissociation of $\mathrm{N}_2 \mathrm{O}_4$ was found to $50 \%$. Which of the following is correct at equilibrium ? (a) $\frac{1}{2}[\mathrm{NO}]=\frac{3}{2}\left[\mathrm{O}_2\right]$ (b) $2\left[\mathrm{~N}_2 \mathrm{O}_4\right]=[\mathrm{NO}]+\frac{3}{2}\left[\mathrm{O}_2\right]+\left[\mathrm{N}_2 \mathrm{O}_5\right]$ (c) $[\mathrm{NO}]+\left[\mathrm{O}_2\right]=\left[\mathrm{N}_2 \mathrm{O}_4\right]+\left[\mathrm{N}_2 \mathrm{O}_5\right]$ (d) $\frac{1}{2}\left[\mathrm{~N}_2 \mathrm{O}_5\right]+\left[\mathrm{O}_2\right]=\frac{1}{2}[\mathrm{NO}]$

Two moles of $\mathrm{N}_2 \mathrm{O}_4$ is heated to form NO and $\mathrm{O}_2$. As soon as NO and $\mathrm{O}_2$ are formed they react to form $\mathrm{N}_2 \mathrm{O}_5$. Two equilibria

$$
\begin{aligned}
\mathrm{N}_2 \mathrm{O}_4 & \rightleftharpoons 2 \mathrm{NO}+\mathrm{O}_2 \\
2 \mathrm{NO}+\frac{3}{2} \mathrm{O}_2 & \rightleftharpoons \mathrm{~N}_2 \mathrm{O}_5
\end{aligned}
$$

Are simultaneously established. At equilibrium, the degree of dissociation of $\mathrm{N}_2 \mathrm{O}_4$ was found to $50 \%$.
Which of the following is correct at equilibrium ?
(a) $\frac{1}{2}[\mathrm{NO}]=\frac{3}{2}\left[\mathrm{O}_2\right]$
(b) $2\left[\mathrm{~N}_2 \mathrm{O}_4\right]=[\mathrm{NO}]+\frac{3}{2}\left[\mathrm{O}_2\right]+\left[\mathrm{N}_2 \mathrm{O}_5\right]$
(c) $[\mathrm{NO}]+\left[\mathrm{O}_2\right]=\left[\mathrm{N}_2 \mathrm{O}_4\right]+\left[\mathrm{N}_2 \mathrm{O}_5\right]$
(d) $\frac{1}{2}\left[\mathrm{~N}_2 \mathrm{O}_5\right]+\left[\mathrm{O}_2\right]=\frac{1}{2}[\mathrm{NO}]$

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of the reactants and products over time. This concept is crucial in analyzing how interrelated reactions achieve balance and how the system responds to changes in conditions.

Reaction Stoichiometry

Reaction stoichiometry is the quantitative relationship between reactants and products as given by the balanced chemical equation. It lays the groundwork for determining the relationships among species in a reaction, thus enabling the construction of concentration relationships and mass balance equations in equilibrium problems.

Degree of Dissociation

The degree of dissociation indicates the fraction or percentage of a reactant that is converted into products in a reversible reaction. It plays an important role in calculating the equilibrium concentrations of the involved species and understanding the extent of reaction progress.

Simultaneous Equilibria

Simultaneous equilibria involve more than one equilibrium reaction occurring at the same time within a system, typically sharing one or more common species. Understanding how these equilibria interact is critical for correctly applying stoichiometric and mass balance constraints to predict the concentrations of all species at equilibrium.

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