Nitrogen monoxide and chlorine were mixed in a 2:1 2:1\,2:1 mole ratio and allowed to reach equilibrium in a sealed vessel at a temperature of 600 K. The equation for the reaction is:
2NO(g)+Cl2(g)⇌2NOCl(g) 2\text{NO(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons 2\text{NOCl(g)} 2NO(g)+Cl2(g)⇌2NOCl(g)When equilibrium was reached, the total pressure in the vessel was 360 kPa and the mole fraction of NOCl(g)\text{NOCl(g)}NOCl(g) in the mixture was 0.40. Calculate the partial pressure of each gas in this equilibrium mixture.
Give an expression for the equilibrium constant (KpK_pKp) for this reaction.
In a different equilibrium mixture, under different conditions, the partial pressures of the gases were: p(NO)=1.50×102 kPap(\text{NO}) = 1.50 \times 10^2\text{ kPa}p(NO)=1.50×102 kPa, p(Cl2)=2.40×102 kPap(\text{Cl}_2) = 2.40 \times 10^2\text{ kPa}p(Cl2)=2.40×102 kPa, and p(NOCl)=1.80×102 kPap(\text{NOCl}) = 1.80 \times 10^2\text{ kPa}p(NOCl)=1.80×102 kPa. Calculate the value of the equilibrium constant (KpK_pKp) for this reaction and give its units.
The enthalpy change for the forward reaction is -76 kJ mol-1. State the effect, if any, of an increase in temperature on the value of Kp K_p\,Kp for this reaction. Justify your answer.