Question

Various nitrogen oxides, as well as sulfur oxides, contribute to acidic rainfall through complex reaction sequences. Nitrogen and oxygen combine during the high-temperature combustion of fuels in air to form nitrogen monoxide gas, which reacts with more oxygen to form nitrogen dioxide gas. In contact with water vapor, nitrogen dioxide forms aqueous nitric acid and more nitrogen monoxide. (a) Write balanced equations for these reactions.

Answer 1

$\begin{aligned}&\mathrm{N}_2(g)+\mathrm{O}_2(g) \longrightarrow 2 \mathrm{NO}(g) \\&2 \mathrm{NO}(g)+\mathrm{O}_2(g) \longrightarrow 2 \mathrm{NO}_2(g) \\&3 \mathrm{NO}_2(g)+\mathrm{H}_2 \mathrm{O}(g) \longrightarrow 2 \mathrm{HNO}_3(a q)+\mathrm{NO}(g)\end{aligned}$

The above is balanced equations for the reactions mentioned in the question.

What is balanced equation?

A balanced reaction equation demonstrates atom conservation by displaying not only the several forms the reactants might take but also their amounts and quantities.

For instance, H + O H0 is the equation for the reaction between hydrogen and oxygen in its most basic form.

However, water is H₂O (the reaction proportion is 2:1, not 1:1), hence the equation needs an adjust: H₂ + O → H₂O.

However, due to the fact that oxygen occurs as diatomic molecules (O2), that is not yet the correct, final form. So put that: H2 + O2 H2O.

The amount of atoms on the left and right sides do not match, so this is not good enough. It is also not yet in balance. The coefficients must be changed in order for the right numbers to appear everywhere:

2H₂ + O₂ → 2H₂O

It works like this: on the left, there are 4 H atoms and 2 O atoms, and on the right, there are 4 H atoms and 2 O atoms.

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