Do not include states of matter in the equation. Use uppercase for the first character in the element and lowercase for the second character. Exercise \(\PageIndex{1}\) Interpret this balanced chemical equation in terms of moles. Do not include states of matter in the equation. References. Tetraphosphorus decoxide, also known as diphosphorous pentoxide, is a white powder a.f.a.i.k. and a very powerfull desiccant forming phosphoric aci. The balanced equation will appear above. Tetraphosphorous decoxide (P 4 O 10 (Click in the answer box to activate the palette.) P 4O 10(s) + 6H 2O(l) → 4H 3PO 4(aq) Imagine that it is your job to design an industrial procedure for running this reaction. The table shows element percentages for P 4 O 10 (tetraphosphorus decaoxide). We would speak of this equation as "one mole of molecular phosphorus reacts with five moles of elemental oxygen to make one mole of tetraphosphorus decoxide." B) Phosphine, combusts in oxygen gas to form gaseous water and solid tetraphosphorus decoxide. Element % O: 56.36: P: 43.64: Isotope pattern for P 4 O 10. Now let’s assume that you have been transferred to the division responsible for the 10.1 Equation Stoichiometry 415 The ratio of moles of P 4O 10 to moles of P (which came from the subscripts in the chemical formula, P 4O 10) provided the key conversion factor that allowed us to convert from units of phosphorus to units of tetraphosphorus decoxide. Determine the number of moles of P 4 O 10 required to produce 5.80 moles of phosphoric acid. Write a balanced chemical equation based on the following description: solid tetraphosphorus decoxide can be synthesized from solid tetraphosphorus (P₄) and oxygen gas. ----- B) Determine the number of moles of P4O10 required to produce 4.40 moles of phosphoric acid. phosphorus + oxygen -- tetraphosphorous decoxide. A) Tetraphosphorous decoxide(P4O10) reacts with water to produce phosphoric acid. mol ) reacts with water to produce phosphoric acid. Write the balanced equation for this reaction. Convert the description into a balanced equation: A) When sulfur trioxide gas reacts with water, a solution of sulfuric acid forms. The chart below shows the calculated isotope pattern for the formula P 4 O 10 with the most intense ion set to 100%. ----- C) Determine the number of moles of water required to produce 4.40 moles of phosphoric acid. P+O ---> 3P + 10O so clearly that is not ballanced, so on the other side add a 3 in front of the P and a 10 in front of the O Determine the empirical formula of the oxide. Phosphorus is just P and Oxygen is just O tetra=3 dec=10. When 0.422 g of phosphorus is burned, 0.967 g of a white oxide (a compound of phosphorus and oxygen) is obtained. 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