QuestionJuly 6, 2025

Estimate Delta H for the reaction. 2Cl-N-Clarrow Nequiv N+3Cl-Cl Delta H=square kJ

Estimate Delta H for the reaction. 2Cl-N-Clarrow Nequiv N+3Cl-Cl Delta H=square kJ
Estimate Delta H for the reaction.
2Cl-N-Clarrow Nequiv N+3Cl-Cl
Delta H=square kJ

Solution
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Answer

\Delta H = 1271 \text{ kJ} Explanation 1. Identify Bond Energies Use bond energies: Cl-N-Cl (average) = 200 kJ/mol, N\equiv N = 945 kJ/mol, Cl-Cl = 242 kJ/mol. 2. Calculate Total Energy of Reactants Two Cl-N bonds: 2 \times 200 = 400 kJ/mol. 3. Calculate Total Energy of Products One N\equiv N bond and three Cl-Cl bonds: 945 + 3 \times 242 = 945 + 726 = 1671 kJ/mol. 4. Calculate \Delta H \Delta H = \text{Energy of products} - \text{Energy of reactants} = 1671 - 400 = 1271 kJ/mol.

Explanation

1. Identify Bond Energies<br /> Use bond energies: $Cl-N-Cl$ (average) = 200 kJ/mol, $N\equiv N$ = 945 kJ/mol, $Cl-Cl$ = 242 kJ/mol.<br /><br />2. Calculate Total Energy of Reactants<br /> Two $Cl-N$ bonds: $2 \times 200 = 400$ kJ/mol.<br /><br />3. Calculate Total Energy of Products<br /> One $N\equiv N$ bond and three $Cl-Cl$ bonds: $945 + 3 \times 242 = 945 + 726 = 1671$ kJ/mol.<br /><br />4. Calculate $\Delta H$<br /> $\Delta H = \text{Energy of products} - \text{Energy of reactants} = 1671 - 400 = 1271$ kJ/mol.
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