At 250°C the equilibrium constant (Kp) for the reaction below is 1.81. PCl5(g) PCl3(g) + Cl2(g) Sufficient PCl5 is put into a vessel to give an initial pressure of 2.75 atm at 250°C. What will be the final pressure at this temperature after the system has reached equilibrium?

the partial pressure of the at equilibrium is 1.25 atm

Explanation:

Initial pressure of the

The value of the equilibrium constant =

Initially

2.75 atm      0       0

At equilibrium

(2.74- x)      x         x

The expression for for the given reaction

we get:

Pressure of the at equilibrium :

Hence, the partial pressure of the at equilibrium is 1.25 atm

in the analysis of systems that involve fluid flow, we frequently encounter the combination of properties u and pv.

b) nuclear ive learned that in a pedtrodic table