How many grams of NO are required to produce 145 g of N₂ in the following reaction?
4NH₃(g) + 6NO(g) → 5N₂(g) + 6H₂O(l)

Question

How many grams of NO are required to produce 145 g of N₂ in the following reaction? 4NH₃(g) + 6NO(g) → 5N₂(g) + 6H₂O(l)

Quizplus · Accepted Answer

The molar mass of N₂ is 28 g/mol, so 145 g of N₂ is 145/28 = 5.18 moles. According to the balanced equation, 5 moles of N₂ are produced from 6 moles of NO. Therefore, 5.18 moles of N₂ require (6/5) * 5.18 = 6.216 moles of NO. The molar mass of NO is 30 g/mol, so 6.216 moles of NO is 6.216 * 30 = 186.48 g, approximately 186 g.

How Many Grams of NO Are Required to Produce 145