An equilibrium mixture of pcl 5 ( g ) , pcl 3 ( g ) , and cl 2 ( g ) has partial pressures of 217.0 torr, 13.2 torr, and 13.2 torr, respectively. a quantity of cl 2 ( g ) is injected into the mixture, and the total pressure jumps to 263.0 torr. the appropriate chemical equation is pcl 3 ( g ) + cl 2 ( g ) − ⇀ ↽ − pcl 5 ( g ) calculate the new partial pressures after equilibrium is reestablished.

The new partial pressures of when equilibrium is re-established are 223.4 torr, 6.82 torr and 26.4 torr respectively.

Explanation:

For the given chemical reaction:

The expression of for above reaction follows:

        ........(1)

We are given:

Putting values in above equation, we get:

Now we have to calculate the new partial pressure of .

The reaction is re-established and proceed to right direction by Le-Chatelier's principle to cancel the effect of addition of .

Now, the equilibrium is shifting to the reactant side. The equation follows:

Initial:             13.2         32.8            217.0

At eqm:         13.2-x      32.8-x         217.0+x

Putting values in expression 1, we get:

Neglecting the 40.4 value of 'x'  because pressure can not be more than initial partial pressure.

Thus, the value of 'x' will be, 6.38 torr.

Now we have to calculate the new partial pressures after equilibrium is reestablished.

Partial pressure of = (217.0+x) = (217.0+6.38) = 223.4 torr

Partial pressure of = (13.2-x) = (13.2-6.38) = 6.82 torr

Partial pressure of = (32.8-x) = (32.8-6.38) = 26.4 torr

Hence, the new partial pressures of when equilibrium is re-established are 223.4 torr, 6.82 torr and 26.4 torr respectively.