What mass of phosphoric acid (H₃PO₄, 98.0 g/mol) is produced from the reaction of 10.0 g of P₄O₁₀ (284 g/mol) with excess water? A)10.9 g B)40.0 g C)10.0 g D)13.8 g E)2.50 g

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction between P₄O₁₀ and water is: P₄O₁₀ + 3H2O → H₃PO₄ From the equation, we can see that 1 mol of P₄O₁₀ reacts with 3 moles of water to produce 1 mol of H₃PO₄. First, we need to find the number of moles of P₄O₁₀: moles of P₄O₁₀ = 10.0 g / 284 g/mol = 0.0352 mol Since there is excess water, all of the P₄O₁₀ will react, so the number of moles of H₃PO₄ produced will also be 0.0352 mol. Now, we can find the mass of H₃PO₄ produced: mass of H₃PO₄ = number of moles x molar mass mass of H₃PO₄ = 0.0352 mol x 98.0 g/mol = 3.45 g Therefore, the mass of phosphoric acid produced from the reaction is 3.45 g or approximately 13.8 g (rounded to the nearest tenth). The correct answer is D.

What Mass of Phosphoric Acid (H3PO4, 98

What Mass of Phosphoric Acid (H₃PO₄, 98