(a)[1]
State the name of the industrial process used to produce sulfuric acid.
(b(i))[2]
Describe two ways sulfur dioxide can be obtained.
(b(ii))[2]
State two characteristics of an equilibrium.
(b(iii))[3]
State the usual conditions and name the catalyst used when sulfur dioxide is converted to sulfur trioxide.
(b(iv))[4]
Complete Table 3.1 to show the effect, if any, when the following changes are applied to the conversion of sulfur dioxide to sulfur trioxide. Only use the words increases, decreases or no change.
(b(v))[3]
Explain in terms of collision theory why reducing the temperature lowers the rate of the forward reaction.
(c)[2]
Determine the oxidation number of S atoms in $\text{SO}_4^{2-}$ ions. Show your working in full.