Problem: Consider the following reaction:H2O(g) + Cl 2O(g) → 2HOCl(g)     K 298 = 0.090For Cl2O(g),       ΔG°f = 97.9 kJ/mol       ΔH°f = 80.3 kJ/mol           S° = 266.1 J/K • molb. Use bond energy values from the following table to estimate ΔH° for the reaction.

FREE Expert Solution

To calculate the ΔH°rxn using bond energies, we’re going to use the following equation:

H°rxn=H°products-H°reactants


Balanced Reaction:  H2O(g) + Cl 2O(g) → 2HOCl(g)

*always make sure that the given reaction is balanced


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Problem Details

Consider the following reaction:

H2O(g) + Cl 2O(g) → 2HOCl(g)     K 298 = 0.090

For Cl2O(g),
       ΔG°f = 97.9 kJ/mol
       ΔH°f = 80.3 kJ/mol
           S° = 266.1 J/K • mol

b. Use bond energy values from the following table to estimate ΔH° for the reaction.

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