Answer to Question #118750 in Chemistry for amanda

Question

Apply Le Chatelier’s principle to predict whether, and in which direction, the following
established equilibrium would be shifted by the changes imposed:

2CO(g) + O2(g) <--> 2CO2(g) + heat energy

a) temperature is increased
b) vessel pressure is decreased
c) oxygen is removed
d) platinum catalyst is added
e) carbon monoxide is removed

Answer 1

According to the Le Chatelier’s principle, the equilibrium shift must counteract the change of the conditions. Therefore:

a) as the temperature is increased, the equilibrium will shift in order to consume the extra heat. As the heat is consumed when CO is produced, the equilibrium will shift to the left.

b) when the vessel pressure is decreased: the equilibrium shifts to compensate the action (to increase the pressure) by increasing the number of the moles of gaseous substances. The number of the moles of a gas is higher on the left side. Therefore, the equilibrium will shift to the left.

c) oxygen is removed: to compensate this, the equilibrium will shift to the left (to produce more oxygen).

d) platinum catalyst is added: the addition of catalyst affect only the kinetics of the reaction, but not the equilibrium. The equilibrium will not shift.

e) carbon monoxide is removed: to compensate this, the equilibrium will shift to the left (to produce more carbon monoxide).