“Synthesis gas” can be produced by the catalytic re-forming of methane with steam. The reactions are:

CH₄(g) + H₂O(g) → CO(g) + 3H₂g)                CO(g) + H₂O(g) → CO₂(g) + H₂(g)

Assume equilibrium is attained for both reactions at 1 bar and 1300 K.

(a) Would it be better to carry out the reaction at pressures above 1 bar?
(b) Would it be better to carry out the reaction at temperatures below 1300 K?
(c) Estimate the molar ratio of hydrogen to carbon monoxide in the synthesis gas if the feed consists of an equimolar mixture of steam and methane.
(d) Repeat part (c) for a steam-to-methane mole ratio in the feed of 2.
(e) How could the feed composition be altered to yield a lower ratio of hydrogen to carbon monoxide in the synthesis gas than is obtained in part (c)?
(f) Is there any danger that carbon will deposit by the reaction 2CO → C + CO₂ under conditions of part (c)? Part (d)? If so, how could the feed be altered to prevent carbon deposition?