2mg(s) + o2(g) → 2 mgo(s) δh = -1204 kj
determine which statement is true regarding the reaction above.
a) the reaction is endothermic; the products have a lower total bond energy than the reactants.
b) the reaction is endothermic; the products have a higher total bond energy than the reactants.
c) the reaction is exothermic; the products have a lower total bond energy than the reactants.
d) the reaction is exothermic; the products have a higher total bond energy than the reactants.

Answer is C because since you are forming bonds, energy is released (exothermic). Since it is exothermic, the products will have lower energy than the reactants.

answer: i dont know the answer but this might

explanation:

l

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.