For the following reaction at 600. K, the equilibrium constant, Kp, is 11.5. PCl5(g) PCl3(g) + Cl2(g) Suppose that 2.21...

Question

Question

For the following reaction at 600. K, the equilibrium constant, K_p, is 11.5.

PCl₅(g) equilibrium reaction arrow PCl₃(g) + Cl₂(g)

Suppose that 2.210 g of PCl₅ is placed in an evacuated 535 mL bulb, which is then heated to 600. K.

(a)

What would be the pressure of PCl₅ if it did not dissociate?

(b)

What is the partial pressure of PCl₅ at equilibrium?

(c)

What is the total pressure in the bulb at equilibrium?

(d)

What is the degree of dissociation of PCl₅ at equilibrium?

Answer 1

Answer #1

(book) € PV=nRT p(0.5356) =(2.2109/208-22g/mol) (0108206 Latim / molik) p20.976 atm 6 xp = ppd x Pelz/Pds ® 115=(w3(x)/(0.976

Answer 2

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