Please see the attached file for the fully formatted problem(s).
Hydrogen gas is 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 I bar and 800 K.
(a) Would there be any advantage to 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.
Molar ratio of an equilibrium mixture is calculated from mole percent data.