Question

What is nitrogen monoxide gas that reacts with oxygen gas to produce nitrogen dioxide gas? Write a balanced chemical equation for this reaction?

Answer 1

Hint: We know that the answer for this question lies in finding the molecular formulas for the reactants and products of the given reaction. The oxidation of nitric oxide is giving nitrogen dioxide gas whose molecular formula is $N{{O}_{2}}.$

Complete answer:
A chemical equation represents the substances that are involved in a chemical reaction i.e. reactants and products. The balanced chemical equation is the one that has the same number of atoms on both sides of a reaction. To balance the reaction, we can use the law of conservation of mass. Hit and trial method is used to balance the number of atoms on both, left and right side of the reaction. The mass of products in a chemical reaction must be equal to the mass of reactants.
Now to balance a chemical reaction there are so many methods. First, write down the oxidation and reduction reaction from the given reaction.
Then balance the number of oxygen and hydrogen of the oxidation and reduction reaction. Add to make an equal number of hydrogen and add water to make an equal number of oxygen’s.
Then balance the charge of each oxidation and reduction reaction by the electron.
After that multiply the number with the reaction to make an equal number of electrons in each reaction.
Finally, summarize the reaction to establish a balanced reaction.
This is the balanced chemical equation involving the reaction of Nitrogen gas and Oxygen gas leading to the formation of Nitrogen Monoxide gas. As per the balanced Equation: One mole of Nitrogen reacts with one mole of Oxygen in presence of heat to produce 2 moles of Nitrogen Monoxide.
$N{{O}_{(g)}}+\dfrac{1}{2}{{O}_{2(g)}}\xrightarrow{catalysis}N{{O}_{2(g)}}$
This is the only method to produce oxides of Nitrogen by heating procedure. The reaction environment temperature has to be at least \[2000\text{ }K\] to produce Nitrogen Monoxide.

Note:
Remember that in the above reaction two moles of nitric oxide is being oxidized with one mole of oxygen to form two moles of nitrogen dioxide. These molecules have been identified as follows. Nitric oxide or Nitrogen monoxide: $NO,$ Nitrogen dioxide: $N{{O}_{2}}$