2 NOCl (g)<- ->2 NO (g)+Cl2 (g) Kp = 6.8x10^-19 at 590.0K Delta H^o = +276.3kJ/mol
a) Write the equilibrium expression for the pressure constant, Kp.
b) Gaseous NOCl is added to an evacuated 1.23 L container kept at 590.0K until the pressure inside the container reaches 1.15 atm. Find the partial pressures of each gas when the system reaches equilibrium.
c) Find Kc for this process at 590.0K.
d) Find the change in free energy, Delta G^o 590.0K, for this system at 590.0 K.
e) Does this system contain mostly reactants or mostly products at equilibrium? Justify your answer.
f) In what way can the system be manipulated in order to increase the value of the equilibrium constant, Kp? Justify your answer.
g) What is the equilibrium constant, Kp, for 2 NO (g) + Cl2 (g) <- -> 2 NOCL (g) at 590.0 K? Justify your answer with calculations.
h) Suppose the process on the system was increased. In which direction would the reaction proceed? Justify your answer.
i) The three gases were injected into a separate container at 590.0K and their partial pressures were found to be P (NOCl) =1.2 atm, P(Cl2) = 1.2 atm, and P(NO) = 0.19 atm. Is the system at equilibrium? If not, in which direction is the reaction proceeding? Justify your answers.