Question

Use the reaction and bond information to answer the question. C2H6 → C2H4 H2 Reactant bond energies: H–C = 413 kJ/mol, C–C single bond = 347 kJ/mol Product bond energies: H–C = 413 kJ/mol, C=C double bond = 614 kJ/mol, H–H = 432 kJ/mol Based on the bond energies, is this reaction endothermic or exothermic? Why or why not?.

Answer 1

The energy of the reactant has been higher than the energy of the product, Thus, the reaction has been an exothermic reaction.

Bond energy has been defined as the chemical energy possessed by the bonds in the chemical structure. The energy has been conserved in the chemical reaction.

Is the reaction endothermic or exothermic?

In the reaction in which bond energy of the reactant has been higher than the product, it has been an exothermic reaction.

In the reaction in which the bond energy of the product is higher than the reactant, it has been an endothermic reaction.

In the given reaction

$\rm C_2H_6\;\rightarrow\;C_2H_4\;+\;H_2$

The bond energies of reactant has been:

• H-C bond = 413 kJ/mol
• C-C bond = 347 kJ/mol

The total bond energy of the reactant has been:

$\rm Reactant=6\;\times\;H-C\;bond\;+\;C-C\;bond \\Reactant=6\;\times\;413+347\;kJ/mol\\Reactant=2,825\;kJ/mol$

The total bond energy of the reactant has been 2,825 kJ/mol.

The bond energies of product has been:

• H-C = 413 kJ/mol
• C=C = 614 kJ/mol
• H-H = 432 kJ/mol

The total bond energy of the product has been:

$\rm Product=4\;\times\;H-C\;bond\;+\;C=C\;bond\;+\;H-H\;bond\\Product=4\;\times\;413\;+\;614\;+\;432\;kJ/mol\\Product=2,698\;kJ/mol$

The total bond energy of the product has been 2,698 kJ/mol.

The energy of the reactant has been higher than the energy of the product, Thus, the reaction has been an exothermic reaction, as energy can neither be created nor be destroyed. It has been conserved in the chemical reaction.

Learn more about exothermic reaction, here:

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