Biochemistry (Metabolism and Energy)

First start by balancing the chemical equation:

2C2H6 + 702 -> 4CO2 + 6H2O

Next, calculate the net energy change. How many C-H, C-C bonds are there in the first reactant, O=O bonds? How many C=O bonds in the product, H-O?

2 * [ 6 (413) + 2 (347) ] + 7 * [ 498 ] => 4 * [ 2 (745) ] + 6 * [ 2 (467) ]

9830 => 11564

Therefore, the energy released by the formation of bonds in the products is greater than the energy added by breaking the bonds in the reactants. The energy released is:

11564 - 9830 = 1734

One mole of ethane molecule has a mass of 30.07 g/mol, so the energy content per gram is: 57.66 KJ/g of ethane

The overall oxidation reaction releases energy; therefore, the oxidation of ethane is an exothermic reaction.

Thank you so much

You're welcome, but please double check my calculation. Every textbook registers different numbers. I believe the table that corresponds to your textbook is shown below

Yar. It's almost the same and was really helpful. Tq again