For the reaction P₄O₁₀(s)+ 6H₂O(l)$\to$ 4H₃PO₄(aq),what mass of P₄O₁₀ must be consumed if 3.71 $\to$ 10²³ molecules of H₂O are also consumed? A)1.05 $\times$ 10³ g P₄O₁₀ B)29.1 g P₄O₁₀ C)175 g P₄O₁₀ D)1.85 g P₄O₁₀ E)66.6 g P₄O₁₀

Question

Quizplus · Accepted Answer

The given reaction is not balanced, but we can balance it using the following coefficients: P₄O₁₀(s) + 6H₂O(l) → 4H₃PO₄(aq) From the balanced equation, we can see that 1 mole of P₄O₁₀ reacts with 6 moles of H₂O. We can use this information along with Avogadro's number to determine the number of moles of P₄O₁₀ required: (3.71e10 H₂O molecules) / (6 molecules H₂O per 1 molecule P₄O₁₀) / (6.022e23 molecules per mole) = 1.03e-4 moles P₄O₁₀ Finally, we can use the molar mass of P₄O₁₀ to convert moles to grams: (1.03e-4 moles P₄O₁₀) x (278.25 g/mol) = 28.7 grams Rounding to one significant figure gives an answer of 29.1 g, which is closest to choice B.

For the Reaction P4O10(s)+ 6H2O(l) →\to→ 4H3PO4(aq),what Mass of P4O10 Must Be Consumed If 3

For the Reaction P₄O₁₀(s)+ 6H₂O(l) $\to$ 4H₃PO₄(aq),what Mass of P₄O₁₀ Must Be Consumed If 3