Problem: Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction:2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(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:

H°rxn=H°products-H°reactants


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:

2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(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.

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

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