Using lechâtelier’s principle, determine whether the reactants or products are favored and the direction of the shift in equilibrium (left or right) in the following examples. 2co(g) + o2(g)  2co2(g) + heat a. remove o2 b. lower the temperature c. add co d. remove co2 e. decrease pressure

a. right

b. right

c. left

d. left

e. left

Explanation:

a. When you remove O2 that means that the reactant side is lacking in an O2 so the equilibrium shifts to the product side.

b. This is an exothermic reaction, because heat is on the products side. So since you are decreasing temperature, then it would shift toward your right.

c. WHen you add CO you are adding more to the reactants side therefore the equilibrium would shift toward the left.

d. When you remove CO2 that means that there is a lack of CO2, therefore the equilibrium would shift to the left.

e. When you decrease pressure, you are increasing in volume. So when you look at volume, if it is increasing you look at larger moles, and if it is decreasing you look at smaller moles. In this case, it is increasing therefore it would shift to the left.