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Question 3
Consider the reaction between hydrogen and oxygen as described by the equation
2H2(g) + O2(g) → 2H2O(g); ΔH = -484 kJ mol-1
The ΔH value indicates that
A.
the chemical bonds within two hydrogen molecules and one oxygen molecule are stronger than the chemical bonds within two water molecules.
B.
the chemical bonds within two hydrogen molecules and one oxygen molecule are weaker than the chemical bonds within two water molecules.
C.
there are fewer chemical bonds in two water molecules than there are in two hydrogen molecules and one oxygen molecule.
D.
water has a higher boiling temperature that either hydrogen or oxygen.

The answers say it's B but I thought it was A.

Here is its description:
Question 3
B.
Exothermic reactions release energy and so the energy content of the product molecules is lower than the energy content of the reactant molecules. This is consistent with the bonds (in total) within the product molecules (2 H2O molecules) being stronger than the bonds (in total) within the reactant molecules (2 H2 molecules and 1 O2 molecule)
There is also evidence for this in that the activation energy for the reverse reaction is greater as indicated on the energy profile for an exothermic reaction.

Any thoughts/explanations?

[luken93]

If it is exothermic, it means that energy is released when the two water form. Thus, they have less energy and hence more stable because they are in a lower energy state = the bonds are stronger in the water molecules than the reactants.