Is this reaction predicted to favor the products at low temp, at high temp, or both? support your answer.

Question

Mg(s) 1/2O2(g) >> MgO(s)

Delta H^0 = -601.70kJ

Answer 1

The enthalpy change is massive and favourable. So you can be confident that the reaction is favoured at all temperatures until the temperature becomes really high (how high?  You would need to know the entropy of reaction, which is unfavourable because you are losing the freedom of motion of the oxygen gas).

However, since the reaction is exothermic, it will be less favourable at higher temperature.

I am not quite sure what the questioner had in mind, so I can't tell you what counts as the "right" answer, but there  is the scientific information for you.

Answer 2

At high temp.

It is an endothermic reaction. Adding heat favors the forward reaction.

Answer 3

According to Le Chatelier's Principle on systems at equilibrium, if a stress is put on a system at equilibrium, the system will adjust itself to counteract the change. When temperatures are increased, the reaction proceeds in the endothermic direction and when temperatures are decreased, the reaction proceeds in the exothermic direction. The forward reaction is exothermic so when you decrease the temperature, the reaction proceeds to make more products.

So in this reaction, products are favored at low temperatures.