Hydrogen gas can be produced by the reaction of steam with "water gas" that is 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 adsorbed, leaving a product that is mostly hydrogen. The equilibrium conditions are 1 bar and 800K. a) Is there 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 2 mol%CO after cooling to 20C, where the unreacted water 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)