2 Mg (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.

Question

Mario Cooke

Chemistry

2 December, 20:56

2 Mg (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.

+4

Answers (1)

Know the Answer?

Kane Lane · Answer 1

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.