n₂ + 3h₂ → 2nh₃\nhow many grams of nitrogen,\nn₂, would be required to create\n9.3 moles ammonia…

n₂ + 3h₂ → 2nh₃\nhow many grams of nitrogen,\nn₂, would be required to create\n9.3 moles ammonia, nh₃?\nmolar mass n₂: 28.02 g/mol\n? g n₂

n₂ + 3h₂ → 2nh₃\nhow many grams of nitrogen,\nn₂, would be required to create\n9.3 moles ammonia, nh₃?\nmolar mass n₂: 28.02 g/mol\n? g n₂

Answer

Explanation:

Step1: Find moles of (N_2)

From the balanced equation (N_2 + 3H_2\rightarrow2NH_3), the mole ratio of (N_2) to (NH_3) is (1:2). If (n(NH_3)=9.3\space mol), then (n(N_2)=\frac{1}{2}\times n(NH_3)) (n(N_2)=\frac{1}{2}\times9.3\space mol = 4.65\space mol)

Step2: Calculate mass of (N_2)

Use the formula (m = n\times M), where (M(N_2) = 28.02\space g/mol) and (n(N_2)=4.65\space mol) (m(N_2)=4.65\space mol\times28.02\space g/mol) (m(N_2)=4.65\times28.02\space g) (m(N_2)=130.3\space g)

Answer:

(130.3\space g)