2) For the reaction, PCIs(g) = PCI:(g)+ Ch(g) at 327°C, the equilibrium constant, Ke is 0.234. Suppose that 2.082 g PCIS is placed in an evacuated 200 mL bulb, which is then heated to 327°C. (R - 0.082 L atm mol 'K, PCIS= 208.2 g/mol) (a) What would be the pressure of PCI; if it did not dissociate? (b) What is the partial pressure of PCIS at equilibrium? (c) What is the total pressure in the bulb at equilibrium? (d) What is the fraction of PCIs at cquilibrium?

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2) For the reaction,
PCI:(g) = PCl:(g) + Ch(g)
at 327°C, the equilibrium constant, Ke is 0.234. Suppose that 2.082 g PCIIS is placed in an evacuated
200 mL bulb, which is then heated to 327°C. (R = 0.082 L atm mol'K', PCIS = 208.2 g/mol)
(a) What would be the pressure of PCIs if it did not dissociate?
(b) What is the partial pressure of PCIS at equilibrium?
(c) What is the total pressure in the bulb at equilibrium?
(d) What is the fraction of PCIS at cquilibrium?
Transcribed Image Text:2) For the reaction, PCI:(g) = PCl:(g) + Ch(g) at 327°C, the equilibrium constant, Ke is 0.234. Suppose that 2.082 g PCIIS is placed in an evacuated 200 mL bulb, which is then heated to 327°C. (R = 0.082 L atm mol'K', PCIS = 208.2 g/mol) (a) What would be the pressure of PCIs if it did not dissociate? (b) What is the partial pressure of PCIS at equilibrium? (c) What is the total pressure in the bulb at equilibrium? (d) What is the fraction of PCIS at cquilibrium?
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