Question

given the following reaction:

n₂ + 3 h₂ → 2 nh₃

if 10.0 moles of ammonia was created, how many moles of nitrogen gas must have reacted? your answer should include the units and the correct number of significant figures.

○ 2.00 mol n₂

○ 5.00 mol n₂

○ 15.00 mol n₂

○ 20.0 mol n₂

Explanation:

Step1: Analyze the mole ratio

From the balanced chemical equation \(N_{2}+3H_{2}\to2NH_{3}\), the mole ratio of \(N_{2}\) to \(NH_{3}\) is \(1:2\).

Step2: Calculate moles of \(N_{2}\)

Let \(n(N_{2})\) be the moles of \(N_{2}\) and \(n(NH_{3}) = 10.0\space mol\). Using the mole ratio \(\frac{n(N_{2})}{n(NH_{3})}=\frac{1}{2}\), we can solve for \(n(N_{2})\). So \(n(N_{2})=\frac{1}{2}\times n(NH_{3})\). Substitute \(n(NH_{3}) = 10.0\space mol\) into the equation: \(n(N_{2})=\frac{1}{2}\times10.0\space mol = 5.00\space mol\).

Answer:

\(5.00\space mol\space N_{2}\) (corresponds to the second option)