Given the balanced equation 4NH₃(g) + 5O₂(g)$\rightarrow$4NO(g) + 6H₂O(g), if 32.5 g of NH₃react with sufficient oxygen, how many grams of H₂O should form?

Question

Quizplus · Accepted Answer

First, calculate the moles of NH₃: 32.5 g / 17.03 g/mol = 1.91 mol. According to the balanced equation, 4 moles of NH₃ produce 6 moles of H₂O. Therefore, 1.91 moles of NH₃ will produce (1.91 mol NH₃) * (6 mol H₂O / 4 mol NH₃) = 2.865 mol H₂O. Convert moles of H₂O to grams: 2.865 mol * 18.02 g/mol = 51.6 g H₂O.

Given the Balanced Equation 4NH3(g) + 5O2(g) →\rightarrow→ 4NO(g) + 6H2O(g), If 32

Given the Balanced Equation 4NH₃(g) + 5O₂(g) $\rightarrow$ 4NO(g) + 6H₂O(g), If 32