Q. 7.108 - An Introduction to General, Organic, and Biological Chemistry

Question

The equation for the formation of nitrogen oxide is ($7.9$) 

data-custom-editor="chemistry" ${\mathrm{N}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) +90.2 \mathrm{kJ} \to 2\mathrm{NO}\left(\mathrm{g}\right)$

a. Is the formation of data-custom-editor="chemistry" $\mathrm{NO}$ an endothermic or exothermic reaction?

b. Is the energy of the product higher or lower than the energy of the reactants?

Step-by-Step Solution

Answer

(a) Formation of $\mathrm{NO}$ is an endothermic reaction

(b) The energy of the product is higher than the energy of the reactants 

Part (a) Step 1: Given information

We need to find whether the formation of $\mathrm{NO}$ is exothermic or endothermic 

Part (a) Step 2: Explanation

We know that

A reaction in which energy is gained is called an endothermic reaction

And in given $90.2 kJ$ of energy is gained

Therefore, the Formation of data-custom-editor="chemistry" $\mathrm{NO}$ is an endothermic reaction

Part (b) Step 1: Given information

We need to find the energy of the product higher or lower than the energy of the reactants  

Part (b) Step 2: Explanation

We know that

The total energy of reactants is equal to the total energy of products in a reaction

And as the energy on the reactant side is gained separately

Therefore, The energy of the reactants is lower than the energy of the products