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.
2 answers
if you increase either of the reactants concentration, shift to the right. Change in temp? no shifting. Adding CO? shifts to right.
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).
1 answer