Question

. Tetraphosphorus decaoxide (P4010) reacts with H2O to form H2PO4. The balanced equation for this reaction is shown in Equation 11. P4010(s) + 6H2O(l) + 4H3PO4(4) (Eq. 11) Calculate the mass of H3PO4 that could possibly be produced by the reaction of 300 g of P4010 with 100 g of H2O. ning conner(IT)

Answer 1

Given reaction P40% (s) + 6H0 (1) 41₂P 04 (2) Imole P400 reacts with 6 mole Ho and produce 4 mole Hapo 1 mole P4 20 = 284 g/mae 1 mole tho = 184/mol H3PO4 = 989/mol Given data ho 100g P4010 = 300g mole ratio = number of moles from data number of moles from balanced equation number of moles = weight/molar mass 21 010 moles - доо 2849/mol = 1.056 mol mole ratio = 1.056 mol I mo! -11056 kot moles = log = 5.555 mol mole ratio = 5.555 mol 6 mol 0.926

& Least mole ratio ho. Limiting reactant tho. product quantity depends on the 6 moje o — ч юle Pa4 GX 18 Но — 4 x 489 о fo, ə lo8 3 • 40 — 348 3 • fo, Тоо 3 + 0 — — № 4PG :. 348 3 од Ро, * x Too 4 •4 lo84 оно = 362-46 8 с 4Po 1. Mass 4 HP = 362-469 — 3633