The enthalpy change for the reaction, 4H(g) → 2$\mathrm{H_{2}(g)}$ is –869.6 kJ. The dissociation energy of H–H bond is;
- A217.4 kJ
- B– 434.8 kJ
- C+869.6 kJ
- D+ 434.8 kJ
✓ Correct answer: D
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The enthalpy change for the reaction, 4H(g) → 2$\mathrm{H_{2}(g)}$ is –869.6 kJ. The dissociation energy of H–H bond is;
Want the full step-by-step reasoning?
Question ID #395480 · NewNcert