See the attached file.
"Synthesis gas" may be produced by the catalytic reforming of methane with steam:
CH4(g) + H2O(g) ?> CO(g) + 3H2(g)
The only other reaction considered is:
CO(g) + H2O(g) ?> CO2(g) + H2(g).
Assume equilibrium is attained for both reactions at I bar and 1300 K.
(1) Would it he better to carry out the reaction at pressures above 1 bar?
(b) Would it he 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)?
(a). By increasing the pressure above 1 bar, this will cause an equilibrium shift to the side of the reaction in the direction where the number of moles of gas decreases (LeChatelier's Principle). Thus, this will cause a shift to the left, giving a decrease in the amount of synthesis gas. (I am assuming that synthesis gas is H2). Therefore, No is would not be ...
The Feed Composition and Molar Ratio is calculated for a Synthesis Gas reaction.