The principle says if a change occurs at equilibrium, the reaction will shift to "undo" the change.
a. CO is removed, the reaction will go to the right to make more CO.
b) The reaction will shift to the left to make more H2O (g).
g) Not indicated, is the heat of reaction, however, this reaction is endothermic (it takes heat to change methane and steam to make hydrogen gas). So if you increase temp, it will shift to the right. Increasing temp is adding heat.
CH4 (g)+ H2O (g) --->/<---- 3H2 + CO
Use Le Chateliers Principle to explain what will happen to the number of moles of hydrogen at equilibrium when
a) CO is removed
b) Water Vapor is removed
c) Methane is added
d) CO is added
e) Pressure is increased by adding argon gas, but the partial pressure of the reactants and products do not change.
f) The pressure is decreased by opening a valve to a second reaction vessel, which lowers the partial pressures of the reactants and products.
g) The temperature is increased.
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