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# Problem: Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction:2 H3C−CH3(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)Note that the average bond energy for the breaking of a bond in CO2 is 799 kJ/mol. Use average bond energies to calculate ΔHrxn for this reaction.

###### FREE Expert Solution

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

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

Balanced Reaction:  2 H3C−CH(g)  +  7 O(g)   →  4  CO2  (g)  +   6  H2O (g)

*always make sure that the given reaction is balanced

Draw the structure of each compound.

Reactants:

H3C−CH3

• 2:

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###### Problem Details

Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction:

2 H3C−CH3(g) + 7 O2(g) → 4 CO2(g) + 6 H2O(g)

Note that the average bond energy for the breaking of a bond in CO2 is 799 kJ/mol. Use average bond energies to calculate ΔHrxn for this reaction.

Frequently Asked Questions

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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Paliwal's class at Stevens Institute of Technology.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Principles of Chemistry: A Molecular Approach - Tro 4th Edition. You can also practice Principles of Chemistry: A Molecular Approach - Tro 4th Edition practice problems.