Sulfur dioxide and oxygen were mixed in a 2:1 2:1\,2:1 mole ratio and left to reach equilibrium in a sealed flask at a temperature of 700 K. The equation for the reaction is:
2SO2(g)+O2(g)⇌2SO3(g)2\mathrm{SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)}2SO2(g)+O2(g)⇌2SO3(g)
When equilibrium was reached, the total pressure in the flask was 450 kPa and the mole fraction of SO3(g)\mathrm{SO_3(g)}SO3(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(SO2)=1.50×102 kPap(\mathrm{SO_2}) = 1.50 \times 10^2\text{ kPa}p(SO2)=1.50×102 kPa p(O2)=2.50×102 kPap(\mathrm{O_2}) = 2.50 \times 10^2\text{ kPa}p(O2)=2.50×102 kPa p(SO3)=3.00×102 kPap(\mathrm{SO_3}) = 3.00 \times 10^2\text{ kPa}p(SO3)=3.00×102 kPa
Calculate the value of the equilibrium constant (KpK_pKp) for this reaction and give its units.
The enthalpy change for the reaction is -197 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.