Asked by Jean

Consider the equilibrium reaction

CO(g)+H2O(g)⇋CO2(g)+H2(g)
Determine how each change in the left-hand column will stress the system and in which direction the equilibrium reaction will shift in response.
Answered by bobpursley
if you increase either of the reactants concentration, shift to the right. Change in temp? no shifting. Adding CO? shifts to right.
Answered by Olereb48
Don't for get about Pressure-Volume effects. Changes in Pressure-Volume will not affect this reaction b/c molar volumes of gas are equal on both sides of equation. However, Vm(Reactants)>Vm(Products), increasing pressure (decreasing volume) shifts reaction to lower molar volume side; or if pressure is decreased, reaction will shift to the higher molar volume side. If Vm(Reactants)<Vm(Products), shifts will be opposite of Vm(R)>Vm(P).
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