Consider the reaction represented by the equation: 2SO\(_{2(g)}\) + O\(_{2(g)}\)   2SO\(_{3(g)}\). \(\Delta\)H = 188KJ.

(a) Write an expression for the equilibrium constant

(b) Sketch an energy diagram for the forward reaction, showing the profile for the catalyzed and non-catalyzed systems.

(c) state the reason, the effect of the following on the position of equilibrium of the system:

(i) increase in temperature

(ii) increase in pressure;

(iii) removal of some of the SO\(_3\) produced;

(iv) presence of V\(_2\)O\(_5\)

(d)(i) Write equations to show how the sulphur(VI) oxide is converted to tetraoxosulphate(VI) acid in the contact process

(ii) Give two uses of tetraoxosulphate(VI) acid.