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Chemistry · CHEMICAL BONDING AND MOLECULAR STRUCTURE
हिन्दीGiven the bond dissociation enthalpy of \( \text{N}_2(\text{g}) \) is \( 946.0\text{ kJ mol}^{-1} \) and that of \( \text{O}_2(\text{g}) \) is \( 498.0\text{ kJ mol}^{-1} \). If a gaseous mixture contains \( 0.5\text{ mol} \) of \( \text{N}_2 \) and \( 1.5\text{ mol} \) of \( \text{O}_2 \), what is the total energy required to completely dissociate all molecules into isolated gaseous atoms?
Correct answer · Option 2
\( 1220.0\text{ kJ} \)
Explanation
\( E = (0.5 \times 946.0) + (1.5 \times 498.0) = 473.0 + 747.0 = 1220.0\text{ kJ} \).
