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

Question

Quizplus · Accepted Answer

First, identify the correct molecular formulas from the given equation: NH3 (ammonia) reacts with O2 (oxygen) to produce NO (nitric oxide) and H2O (water). Using the molar mass of NH3 (17.03 g/mol), 32.5 g NH3 is equivalent to 32.5 / 17.03 = 1.908 moles of NH3. According to the balanced equation, 4 moles of NH3 produce 6 moles of H2O. Therefore, 1.908 moles of NH3 will produce (1.908 / 4) * 6 = 2.862 moles of H2O. The molar mass of H2O is 18.015 g/mol, so the mass of H2O produced is 2.862 moles * 18.015 g/mol = 51.6 g.

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

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