Question

Using the table of average bond energies, determine the total bond energy for the products in the combustion of ethene: C2H4 + 3 O2 --> 2 CO2 + 2 H2O

Answer 1

Answer:

$B\text{ : }5064\text{ KJ/mol}$

Explanation:

Here, we want to get the total bond energy for the products

On the products side, we have 4 C=O bonds formed and 4 O-H bonds formed

We have the values from the given table above

Thus, we have the energy as the sum of the energy of the bonds

Mathematically, we have that as:

$(4\times\text{ 799 \rparen + \lparen4 }\times467)\text{ = 5,064 KJ/mol}$

We would be having the answer as negative since the process of bond formation is exothermic (heat is given off and enthalpy change value is negative)