To determine how many grams of H₃PO₄ are produced when 100 moles of water react with P₄O₁₀, we first need to look at the balanced chemical equation for the reaction:
P₄O₁₀ + 6 H₂O → 4 H₃PO₄
This equation shows that one mole of P₄O₁₀ reacts with six moles of water to produce four moles of H₃PO₄. According to the equation, 6 moles of water yield 4 moles of H₃PO₄.
Now, if we have 100 moles of water, we can calculate how many moles of H₃PO₄ will be produced:
- First, we find out how many moles of H₃PO₄ can be produced from 100 moles of water using the ratio from the balanced equation:
- From the equation, 6 moles of water produce 4 moles of H₃PO₄, so for 100 moles of water:
Moles of H₃PO₄ = (100 moles of H₂O) * (4 moles of H₃PO₄ / 6 moles of H₂O) = 66.67 moles of H₃PO₄
Next, we need to convert the moles of H₃PO₄ to grams. The molar mass of H₃PO₄ (phosphoric acid) can be calculated as follows:
- 1 phosphorus (P) = 30.97 g/mol
- 4 oxygens (O) = 16.00 g/mol * 4 = 64.00 g/mol
- 3 hydrogens (H) = 1.01 g/mol * 3 = 3.03 g/mol
Adding these together gives:
Molar mass of H₃PO₄ = 30.97 g/mol + 64.00 g/mol + 3.03 g/mol = 98.00 g/mol
Finally, to find the mass of H₃PO₄ produced, we multiply the moles of H₃PO₄ by its molar mass:
Mass of H₃PO₄ = 66.67 moles * 98.00 g/mol = 6533.33 grams
Thus, when 100 moles of water react with P₄O₁₀, approximately 6533.33 grams of H₃PO₄ are produced.