Question

For the reaction below, use the bond energies to calculate the net energy of reaction and state if reaction is exothermic or endothermic reaction with reason(s). 2N≡N + 2O=O 2N=O + 2N= O(N≡N is +946 Kj/mole; O=O is +498 Kj/mole; N=O is -631 Kj/mole).

Answer 1

Net energy of reaction = -5412kJ

Reaction is exothermic

Explanations:

Given the following reaction;

`2N≡N+2O=O\rightarrow2N=O+2N=O`

The net energy of the reaction is expressed as:

`\triangle H=H_p-H_r`

Determine the enthalpy change of the product

`\begin{gathered} H_p=2(-631)+2(-631) \\ H_p=-1262-1262 \\ H_p=-2524kJ \\ \end{gathered}`

Determine the enthalpy change for the reactant

`\begin{gathered} H_r=2(946)+2(498) \\ H_r=1892+996 \\ H_r=2888kJ \end{gathered}`

Determine the net energy for the reaction

`\begin{gathered} \triangle H=-2524kJ-2888kJ \\ \triangle H=-5412kJ \end{gathered}`

Since the net energy of the reaction is negative, hence the reaction will be exothermic (energy is liberated to the surrounding)