# 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:

$\overline{){\mathbf{∆}}{\mathbf{H}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{∆}}{\mathbf{H}}{{\mathbf{°}}}_{{\mathbf{products}}}{\mathbf{-}}{\mathbf{∆}}{\mathbf{H}}{{\mathbf{°}}}_{{\mathbf{reactants}}}}$

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.

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Bond Energy concept. You can view video lessons to learn Bond Energy. Or if you need more Bond Energy practice, you can also practice Bond Energy practice problems.

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What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.