Question

how many grams of nitrogen, n2, would be required to react with 6.25 moles hydrogen, h2? n2 + 3h2 → 2nh3 molar mass n2: 28.02 g/mol ? g n2

Explanation:

Step1: Find moles of \(N_2\)

From the balanced equation \(N_2 + 3H_2
ightarrow2NH_3\), the mole ratio of \(N_2\) to \(H_2\) is \(1:3\).
Let \(n(N_2)\) be the moles of \(N_2\) and \(n(H_2) = 6.25\) mol.
Using the mole - ratio formula \(n(N_2)=\frac{1}{3}n(H_2)\)
\(n(N_2)=\frac{1}{3}\times6.25\space mol=\frac{6.25}{3}\space mol\approx2.083\space mol\)

Step2: Calculate mass of \(N_2\)

The formula for mass \(m = n\times M\), where \(n\) is the number of moles and \(M\) is the molar mass.
Given \(M(N_2)=28.02\space g/mol\) and \(n(N_2)\approx2.083\space mol\)
\(m(N_2)=n(N_2)\times M(N_2)\)
\(m(N_2)=2.083\space mol\times28.02\space g/mol\)
\(m(N_2)\approx58.4\space g\)

Answer:

\(58.4\space g\)