Answer:
42,3g of H₂O
Explanation:
For the reaction:
4NH₃(g) + 5O₂(g) ⟶ 4NO(g) + 6H₂O(g)
62,8 g of NH₃ are:
62,8g×(1mol/17,031g) = <em>3,69 moles of NH₃</em>
62,8 g of O₂ are:
62,8g×(1mol/32g) =<em> 1,96 moles of O₂</em>
For a complete reaction of 1,96 moles of O₂ you need:
1,96mol O₂×(4mol NH₃ / 5molO₂) = 1,57 moles NH₃. As you have 3,69 moles, limiting reactant is O₂.
Assuming a complete reaction, 1,96mol O₂ produce:
1,96mol O₂×(6mol H₂O / 5molO₂) = 2,35 moles of H₂O. In grams:
2,35 moles of H₂O×(18,01g/1mol) = <em>42,3g of H₂O</em>
I hope it helps!
