Hydrogen gas can be produced by the reaction of steam with “water gas,” an equimolar mixture of H₂ and CO obtained by the reaction of steam with coal. A stream of “water gas” mixed with steam is passed over a catalyst to convert CO to CO₂ by the reaction:

H₂O(g)  + CO(g)  →  H₂(g)  +  CO₂(g)

Subsequently, unreacted water is condensed and carbon dioxide is absorbed, leaving a product that is mostly hydrogen. The equilibrium conditions are 1 bar and 800 K.
(a) Is any advantage gained by carrying out the reaction at pressures above 1 bar?
(b) Would increasing the equilibrium temperature increase the conversion of CO?
(c) For the given equilibrium conditions, determine the molar ratio of steam to “water gas” (H₂ + CO) required to produce a product gas containing only 2-mol-% CO after cooling to 20°C, where the unreacted H₂O has been virtually all condensed.
(d) Is there any danger that solid carbon will form at the equilibrium conditions by the reaction

2CO(g)  →  CO₂(g)  + C(s)