Question

For the following reaction at 600. K, the equilibrium constant, Kp is 11.5.
PCl5(g) PCl3(g) + Cl2(g)

Suppose that 3.314 g of PCl5 is placed in an evacuated 460. mL bulb, which is then heated to 600. K.
(a) What would be the pressure of PCl5 be if it did not dissociate?
1 atm
(b) What is the partial pressure of PCl5 at equilibrium?
2Check the number of significant figures. atm
(c) What is the total pressure in the bulb at equilibrium?
3Check the number of significant figures. atm
(d) What is the degree of dissociation of PCl5 at equilibrium?
4%
Would you mind going through how you obtained the answers you have? I don't see how you could come up with 1 atm for (a). Is that the right answer?

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