An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 Torr (at the moment of mixing). The system then re-equilibrates. The appropriate chemical equation is PCl3(g)+Cl2(g) <-->PCl5(g) Calculate the new partial pressures after equilibrium is reestablished in torr

The new partial pressures after equilibrium is reestablished:

Explanation:

At equilibrium before adding chlorine gas:

Partial pressure of the

Partial pressure of the

Partial pressure of the

The expression of an equilibrium constant is given by :

At equilibrium after adding chlorine gas:

Partial pressure of the

Partial pressure of the

Partial pressure of the

Total pressure of the system = P = 263.0 Torr

At initail

(13.2) Torr     (32.8) Torr                        (13.2) Torr

At equilbriumm

(13.2-x) Torr     (32.8-x) Torr                        (217.0+x) Torr

Solving for x;

x = 6.402 Torr

The new partial pressures after equilibrium is reestablished:

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

yes it is balanced