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The reaction PCl3(g)+Cl2(g)= PCl5(g) has Kp= 0.0870 at 300°C. A flask is charged with 0.50 atm PCl3, 0.50 atm Cl2, and 0.20 atm PCl5 at this temperature.
a) Determine in which direction the reaction must proceed in order to reach equilibrium.
b) Calculate the equilibrium partial pressures of each of the three of the gases.
c)What effect will increasing the volume of the system have on the mole fraction of Cl2 in the equilibrium mixture?
d)The reaction is exothermic. What effect will increasing the temperature of the system have on the partial pressure of Cl2 in the equilibrium mixture?
a) Determine in which direction the reaction must proceed in order to reach equilibrium.
b) Calculate the equilibrium partial pressures of each of the three of the gases.
c)What effect will increasing the volume of the system have on the mole fraction of Cl2 in the equilibrium mixture?
d)The reaction is exothermic. What effect will increasing the temperature of the system have on the partial pressure of Cl2 in the equilibrium mixture?