Given the balanced equation 4NH₃(g) + 5O₂(g) $\rightarrow$ 4NO(g) + 6H₂O(g), if 82.0 g of NH₃react with sufficient oxygen, how many grams of NO should form?

Question

Quizplus · Accepted Answer

The molar mass of NH₃ is 17.03 g/mol, so 82.0 g of NH₃ is 82.0 / 17.03 = 4.81 mol. According to the balanced equation, 4 mol of NH₃ produce 4 mol of NO. Therefore, 4.81 mol of NH₃ will produce 4.81 mol of NO. The molar mass of NO is 30.01 g/mol, so 4.81 mol of NO is 4.81 x 30.01 = 144.43 g, which rounds to 145 g.

Given the Balanced Equation 4NH3(g) + 5O2(g) →\rightarrow→ 4NO(g) + 6H2O(g), If 82

Given the Balanced Equation 4NH₃(g) + 5O₂(g) $\rightarrow$ 4NO(g) + 6H₂O(g), If 82