An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217 Torr, 13.2 T

step 1 In answering this question, we're going to be looking at PCL3 plus CL2 to form PCL5. This is a C

An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has...

An equilibrium mixture of $\mathrm{PCl}_{5}(g), \mathrm{PCl}_{3}(g)$, and $\mathrm{Cl}_{2}(g)$ has partial pressures of 217 Torr, $13.2$ Torr, and $13.2$ Torr, respectively. A quantity of $\mathrm{Cl}_{2}(g)$ is injected into the mixture, and the total pressure jumps to 263 Torr. Calculate the new partial pressures after equilibrium is reestablished. The appropriate chemical equation is $$ \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \leftrightharpoons \mathrm{PCl}_{5}(g) $$

An equilibrium mixture of $\mathrm{PCl}_{5}(g), \mathrm{PCl}_{3}(g)$, and $\mathrm{Cl}_{2}(g)$ has partial pressures of 217 Torr, $13.2$ Torr, and $13.2$ Torr, respectively. A quantity of $\mathrm{Cl}_{2}(g)$ is injected into the mixture, and the total pressure jumps to 263 Torr. Calculate the new partial pressures after equilibrium is reestablished. The appropriate chemical equation is
$$
\mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) \leftrightharpoons \mathrm{PCl}_{5}(g)
$$

Key Concepts

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It is essential for relating the changes in concentrations or partial pressures (expressed as changes in moles) as the system shifts to a new equilibrium.

Equilibrium Constant (Kp)

The equilibrium constant expressed in terms of partial pressures (Kp) provides a quantitative measure for the position of equilibrium in gas-phase reactions. Its constant value (at a given temperature) allows one to calculate the shifts in partial pressures when the system is perturbed.

Chemical Equilibrium

Chemical equilibrium occurs in a reversible reaction when the rates of the forward and reverse reactions become equal, resulting in constant concentrations (or partial pressures) of reactants and products. Understanding equilibrium is key to predicting how the system will adjust when disturbed.

Le Chatelier's Principle

Le Chatelier's principle explains that when an equilibrium system is subjected to a change in conditions (such as adding more Cl? gas), the system will shift in the direction that counteracts the change, thereby reestablishing equilibrium at a new set of conditions.

Partial Pressure

Partial pressure is the pressure exerted by an individual gas in a mixture, and according to Dalton's law, the total pressure is the sum of these individual pressures. This concept is critical for analyzing gas-phase equilibria and determining how changes in the amounts of gases affect the overall system.

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