Consider the reaction: SO2Cl2(g) ⟹ SO2(g)+Cl2(g) Kp=2.91 × 10^3at 298 K In a re

step 1 Let's first start by converting the partial pressure of SO2, which is equal to 137 Tor into atmo

Consider the reaction: SO2Cl2(g) ⟹ SO2(g)+Cl2(g) ...

Consider the reaction: \begin{equation}\begin{aligned} \mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \Longrightarrow & \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g) \\ & K_{\mathrm{p}}=2.91 \times 10^{3} \mathrm{at} 298 \mathrm{K} \end{aligned}\end{equation} In a reaction at equilibrium, the partial pressure of $\mathrm{SO}_{2}$ is 137 torr and that of $\mathrm{Cl}_{2}$ is 285 torr. What is the partial pressure of $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ in thismixture?

Consider the reaction:
\begin{equation}\begin{aligned} \mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \Longrightarrow & \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g) \\ & K_{\mathrm{p}}=2.91 \times 10^{3} \mathrm{at} 298 \mathrm{K} \end{aligned}\end{equation}
In a reaction at equilibrium, the partial pressure of $\mathrm{SO}_{2}$ is 137 torr and
that of $\mathrm{Cl}_{2}$ is 285 torr. What is the partial pressure of $\mathrm{SO}_{2} \mathrm{Cl}_{2}$ in thismixture?

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible chemical reaction where the rates of the forward and reverse reactions are equal, leading to constant concentrations or partial pressures of reactants and products. At equilibrium, the system has reached a condition where macroscopic properties remain unaltered over time, although molecular processes continue to occur.

Equilibrium Constant (Kp)

The equilibrium constant in terms of partial pressures, denoted as Kp, quantifies the ratio of the product of the partial pressures of the gaseous products to that of the gaseous reactants at equilibrium, each raised to the power of their stoichiometric coefficients. It is a fundamental parameter that reflects how far a reaction proceeds under a given set of conditions.

Partial Pressure

Partial pressure is the pressure exerted by an individual gas in a mixture of gases, and it contributes to the total pressure of the system. In equilibrium calculations for gaseous reactions, partial pressures are used to determine the position of equilibrium and to relate the measured pressures to the equilibrium constant.

Application of Equilibrium Expressions to Reaction Mixtures

Using the equilibrium constant expression, one can relate the known partial pressures of some components of a reaction mixture to determine the unknown partial pressures of others. This involves substituting the measured partial pressures into the Kp expression and solving for the desired variable, while ensuring that units are consistent throughout the calculation.

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