Chapter 6, Problem 82AE

For the reaction

${\text{PCl}}_{\text{5}}\text{(}g\text{)}\rightleftharpoons {\text{PCl}}_{\text{3}}\text{(}g{\text{)+Cl}}_{\text{2}}\text{(}g\text{)}$

at 600. K, the equilibrium constant is 11.5. Suppose that2.450 g of ${\text{PCl}}_{\text{5}}$ is placed in an evacuated 500.-mL bulb,which is then heated to 600. K.
a. What would the pressure of ${\text{PCl}}_{\text{5}}$ be if it did notdissociate?
b. What is the partial pressure of ${\text{PCl}}_{\text{5}}$ at equilibrium?
c. What is the total pressure in the bulb atequilibrium?
d. What is the degree of dissociation of ${\text{PCl}}_{\text{5}}$ atequilibrium?