Did you mean to type CO(g) + 1/2 O2(g) <------> CO2(g) + 28.3 kJ ?
Le Chatelier's Principle states the equilibrium of a reaction will shift in such a way as to reduce/counter the effects of a change.
a) When the temperature increases, the reaction shifts towards the endothermic side to use the excess heat energy. In this case, the forward reaction is exothermic so it shifts to the left.
b) To counter an increase in a product or reactant, the reaction shifts in the direction that will use up the compound in excess. It shifts to the right.
c) Introducing a catalyst will not shift the equilibrium of a reaction because it only increases the rate by decreasing the required activation energy.
d) An increase in pressure will cause the equilibrium to shift in the direction that reduces the total number of gas molecules so the pressure will decrease. In this case, there are 1.5 molecules on the left and 1 on the right so it will shift to the right.