Exercise 14
At $1000^{\circ} \mathrm{C}$, ammonia gas, $\mathrm{NH}_{3}(\mathrm{~g})$, reacts with oxygen gas to form gaseous nitric oxide, $\mathrm{NO}(\mathrm{g})$, and water vapor. This reaction is the first step in the commercial production of nitric acid by the Ostwald process. Balance the equation for this reaction.

Question

Exercise 14
At $1000^{\circ} \mathrm{C}$, ammonia gas, $\mathrm{NH}_{3}(\mathrm{~g})$, reacts with oxygen gas to form gaseous nitric oxide, $\mathrm{NO}(\mathrm{g})$, and water vapor. This reaction is the first step in the commercial production of nitric acid by the Ostwald process. Balance the equation for this reaction.

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Write the unbalanced chemical equation**: The reaction between ammonia ($\mathrm{NH}_{3}$) and oxygen ($\mathrm{O}_{2}$) to produce nitric oxide ($\mathrm{NO}$) and water ($\mathrm{H}_{2}\mathrm{O}$) is represented by the unbalanced equation: $\mathrm{NH}_{3}(g) + \mathrm{O}_{2}(g) ightarrow \mathrm{NO}(g) + \mathrm{H}_{2}\mathrm{O}(g)$. ‖ ‖ 2 ⋮ **Balance the nitrogen atoms**: There is one nitrogen atom on both sides of the equation, so nitrogen is already balanced. ‖ ‖ 3 ⋮ **Balance the hydrogen atoms**: There are three hydrogen atoms in $\mathrm{NH}_{3}$ and two in $\mathrm{H}_{2}\mathrm{O}$. To balance the hydrogen atoms, we need to have an even number of hydrogen atoms in the water molecules. Therefore, we put a coefficient of 2 in front of $\mathrm{H}_{2}\mathrm{O}$: $\mathrm{NH}_{3}(g) + \mathrm{O}_{2}(g) ightarrow \mathrm{NO}(g) + 2\mathrm{H}_{2}\mathrm{O}(g)$. ‖ ‖ 4 ⋮ **Balance the oxygen atoms**: Now, there are four oxygen atoms on the right side (2 from $\mathrm{NO}$ and 2 from $2\mathrm{H}_{2}\mathrm{O}$) and two on the left side from $\mathrm{O}_{2}$. To balance the oxygen atoms, we need to put a coefficient of 5/2 in front of $\mathrm{O}_{2}$: $\mathrm{NH}_{3}(g) + \frac{5}{2}\mathrm{O}_{2}(g) ightarrow \mathrm{NO}(g) + 2\mathrm{H}_{2}\mathrm{O}(g)$. ‖ ‖ 5 ⋮ **Make all coefficients whole numbers**: To avoid having a fraction as a coefficient, we multiply all coefficients by 2: $2\mathrm{NH}_{3}(g) + 5\mathrm{O}_{2}(g) ightarrow 2\mathrm{NO}(g) + 4\mathrm{H}_{2}\mathrm{O}(g)$. ‖ ∻Answer∻ ⚹ $2\mathrm{NH}_{3}(g) + 5\mathrm{O}_{2}(g) ightarrow 2\mathrm{NO}(g) + 4\mathrm{H}_{2}\mathrm{O}(g)$ ⚹ ∻Key Concept∻ ⚹ Balancing chemical equations ⚹ ∻Explanation∻ ⚹ The coefficients in a balanced chemical equation must be the smallest set of whole numbers that balance all the atoms on both sides of the equation. ⚹◊What is the balanced chemical equation for the reaction between ammonia gas and oxygen gas to form nitric oxide and water vapor at $1000^{\circ} \mathrm{C}$?⍭ Generate me a similar question◊

Sia