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What will be the change in energy for the following reaction? H2(g)+F2(g)→ 2HF Given: To break one mole of H2, energy absorbed is 436 kJ. To break one mole of F2, energy absorbed is 158 kJ. To form one moles of HF, energy released is 568 kJ.

What will be the change in energy for the following reaction? H2(g)+F2(g)→ 2HF Given: To break one mole of H2, energy absorbed is 436 kJ. To break one mole of F2, energy absorbed is 158 kJ. To form one moles of HF, energy released is 568 kJ. Correct Answer -542KJ

So, applying the equation, ∆H = ∑∆H (bonds broken in reactants) − ∑∆H (bonds made in products) ΔH reaction = (436+158)–(2X568) = −542kJ The overall enthalpy of the reaction is negative, i.e., it’s an exothermic reaction where energy is released in the form of heat.

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