The water-gas reaction is used to produce combustible gases from carbon (coal) a

Question

The water-gas reaction is used to produce combustible gases from carbon (coal) and steam: C(s) + H_2O(g) reversiblearrow CO(g) + H_2(g), K_p = 9.7 E - 17 @298K; delta H = 131 kJ What would be the effect on the final equilibrium amount of H_2(g) if a gaseous mixture originally at equilibrium with a large excel of C(s) at 298 K is subjected to the following changes: More H_2O (g) is added A catalyst is added The mixture is transferred to a reaction vessel of greater volume Additional CO(g) is introduced An inert gas is added, which leads to an increase of pressure

Explanation / Answer

a)

more H2O added --> reactants increase, so more products must be formed, shift goes to right

b)

catalyst has NO effect in thermo equilibrium, only in rates, no shift at all

c)

greater volume, implies less pressure....

less pressure favours the least mol formation of gases... which in this case will be produts, sinc there is 2 mol of products whle reagents only 1. shift goes to right

d)

CO added, this is a product, so high products ar epresent, they must turn now to form more reactants

the shift goes to the left

e)

increasing pressure favour least mol formation, so the shift goes toward reactants, i.e. to the left

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