This question is about sulfuric acid and its salts.
The manufacture of sulfuric acid involves the equilibrium
2SO2(g) + O2(g) ⇌ 2SO3(g) ΔrH = −197 kJ mol−1
i)
A catalyst of vanadium(V) oxide is used in this reaction.
State the effect, if any, of the catalyst on the value of the equilibrium constant, Kp.
(1)
ii)
The temperature used for this reaction in industry is 700 K.
Explain, in terms of the equilibrium constant and the equilibrium position, the effect of an increase in temperature on the equilibrium yield of sulfur trioxide.
(2)
iii)
Write the expression for the equilibrium constant, Kp, for this equilibrium.
State symbols are not required.
(1)
iv)
A mixture of 2.00 mol of sulfur dioxide and 1.00 mol of oxygen is allowed to reach equilibrium at 5.00 atm pressure.
1.60 mol of sulfur trioxide is formed.
Calculate the value of Kp.
Include units and give your answer to an appropriate number of significant figures.
(4)