The hydrolysis of P4O10(s) with H2O(l) to produce phosphoric acid, H3PO4(l ):
The balanced chemical Reaction for the hydrolysis of phosphorous pentoxide to form phosphoric acid is
P4O10(s) + 6H2O(l)
4H3PO4(l)
The hydrolysis of P4O10(s) with H2O(l) to produce phosphoric acid, H3PO4(l ):
Phosphoric acid, H3PO4,H3PO4, has some important applications. It can be used to produce fertilizers and it is present in soft drinks. Phosphoric acid can be made from phosphorus in a two step process: Reaction 1: P4+5O2→P4O10P4+5O2→P4O10 Reaction 2: P4O10+6H2O→4H3PO4P4O10+6H2O→4H3PO4 What is the molar mass of phosphoric acid, H3PO4?H3PO4? Report your answer to 3 significant figures. g/mol How many moles of H3PO4H3PO4 can be produced from one mole of P4P4 ? Hint: You need to look at both reaction (1) and reaction (2). Your answer should...
What mass of phosphoric acid can we produce by the following reaction P4(s) + 5 O2(g) + 6 H2O(l) → 4 H3PO4(s) if we have 339.2 g of P4(s), 377.6 g of O2(g), and 310.7 g of H2O(l)?
For the balanced chemical reaction below: P4O10 (g) + 6 H2O (l) → 4 H3PO4 (aq) (a) Calculate the moles of water if there are 9.19 grams of tetraphosphorus decoxide. (b) Calculate the grams of water if there are 0.730 moles of tetraphosphorus decoxide. (c) Calculate the grams of tetraphosphorus decoxide if there are 5.41 grams of H3PO4. (d) Calculate the moles of H3PO4 if there are 0.604 moles of tetraphosphorus decoxide. I am really just unsure how to set...
376.0 g of phosphoric acid, H3PO4, are dissolved in 2.5×103 g of water, H2O. What is the molality (m) of phosphoric acid? your answer should include two significant figures. Provide your answer below:
If a 25.0 mL sample of phosphoric acid, H3PO4, is completely neutralized by 137 mL of 0.100 M KOH, what is the molarity of the phosphoric acid? Given: H3PO4 + 3 KOH → 3 H2O + K3PO4
How many grams of phosphoric acid, H3PO4, must be added to remove (or react with) 15.0 g of rust, Fe2O3? 2H3PO4 (aq) + Fe2O3 (s) à 2FePO4 (s) + 3 H2O (l) STEP 1 15.0 g Fe2O3 -------------------------> _?_ g H3PO4
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH ----> H2O (l) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH ----> H2O (l) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH --> H2O (1) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen. P4 + 5O2 ⟶ P4O10 Calculate the percent yield if 6 g of P4 reacts with 21 g of O2 to yield 4.7 g of P4O10 from the reaction.