Question

gaseous ammonia chemically reacts with oxygen (o₂) gas to produce nitrogen monoxide gas and water vapor. calculate the moles of oxygen needed to produce 0.085 mol of nitrogen monoxide. be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.

Explanation:

Step1: Write the balanced chemical equation

The reaction is $4NH_3(g)+5O_2(g)
ightarrow4NO(g) + 6H_2O(g)$.

Step2: Determine the mole - ratio

From the balanced equation, the mole - ratio of $O_2$ to $NO$ is $\frac{5}{4}$.

Step3: Calculate moles of $O_2$

Let $n_{O_2}$ be the moles of $O_2$ and $n_{NO}=0.085$ mol. Using the mole - ratio, $n_{O_2}=\frac{5}{4}\times n_{NO}$. Substituting the value of $n_{NO}$, we get $n_{O_2}=\frac{5}{4}\times0.085\ mol = 0.10625\ mol$. Rounding to two significant digits, $n_{O_2}=0.11\ mol$.

Answer:

$0.11\ mol$