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]

PPCl3

PPCl2

PPCl5

The new partial pressures after equilibrium is reestablished for :

The new partial pressures after equilibrium is reestablished :

The new partial pressures after equilibrium is reestablished for :

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 for :

The new partial pressures after equilibrium is reestablished :

The new partial pressures after equilibrium is reestablished for :

the answer is a and have a great day

the answer is 0.8m.

by: nicholas