A sample of 45.7 g of tetraphosphorous decoxide (P,O10) reacts with 79.1 g of water to produce phosphoric acid (H, PO,) according to the following balanced equation. P,O10 + 6 H,0 → 4 H,PO, Determine the limiting reactant for the reaction. O P,010 H,O O H, PO, Calculate the mass of H, PO, produced in the reaction. mass of H, PO: Calculate the percent yield of H, PO, if 35.0 g of H, PO, is isolated after carrying out the reaction. percent yield:

A sample of 45.7 g of tetraphosphorous decoxide (P,O10) reacts with 79.1 g of water to produce phosphoric acid (H, PO,) according to the following balanced equation. P,O10 + 6 H,0 → 4 H,PO, Determine the limiting reactant for the reaction. O P,010 H,O O H, PO, Calculate the mass of H, PO, produced in the reaction. mass of H, PO: Calculate the percent yield of H, PO, if 35.0 g of H, PO, is isolated after carrying out the reaction. percent yield:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The rocket boosters of the space shuttle Discovery, launched on July 26, 2005, used a fuel mixture containing primarily solid ammonium perchlorate, NH4ClO4, and aluminum metal. The unbalanced chemical equation for the reaction is given below. (Hint: Balance the elements in the order Cl, H, O, Al, N.) Al(s) + NH4CIO4(s) Al₂O3(s) + AlCl3(s) + H₂O(l) + N₂(g) What is the mass (in kilograms) of NH4ClO4 consumed per kilogram of Al, assuming a percent yield of 87.20%? (Answer with two decimal places.)
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2Mg(s)+O2(g)→2MgO(s)2Mg(s)+O2(g)→2MgO(s) When 10.1 gg of Mg are allowed to react with 10.5 g of O2, 13.4 g of MgO are collected. Determine the theoretical yield for the reaction.
Potassium chlorate, KClO 3 , decomposes upon heating in the presence of a catalyst according to the reaction below. 2KClO 3 (s) 2KCl(s)+3O 2 (g) In a certain experiment 40.0gKClO3 is heated until it completely decomposes. The experiment performed and the oxygen gas is collected and its mass is found to be 10.8g . What is the percent yield? Answer in standard notation, rounded to the nearest tenth of a percent
Please help fill out the table in the attached picture with the given information.
Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2Mg(s)+O2(g)→2MgO(s)2Mg(s)+O2(g)→2MgO(s) When 10.1 gg of Mg are allowed to react with 10.5 g of O2, 13.4 gg of MgO are collected. Determine the limiting reactant for the reaction. Express your answer as a chemical formula.
Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The formula for Epsom salts can be written as MgSO4⋅xH2OMgSO4⋅�H2O, where x� indicates the number of moles of H2OH2O per mole of MgSO4MgSO4. When 5.061 gg of this hydrate is heated to 250 ∘C∘C, all the water of hydration is lost, leaving 2.472 gg of MgSO4MgSO4.
For the following reaction, 0.472 moles of carbon (graphite) are mixed with 0.594 moles of oxygen gas. carbon (graphite)(s) + oxygen(g) → carbon dioxide(g) What is the formula for the limiting reagent? What is the maximum amount of carbon dioxide that can be produced? moles
For the following unbalanced chemical equation, suppose that exactly 1.60 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of CO2 is expected (assuming that the limiting reactant is completely consumed). CS, (1) + 02 (9) → CO2(g) + SO2 (g) Limiting reactant: Mass of CO2 = For the following unbalanced chemical equation, suppose that exactly 1.45 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). NH3 (9) + CO2 (9) → CN, H,O(s) + H2O(1) Limiting reactant: Mass of H2O = b)
Consider the following unbalanced chemical equation: MgS (s) + O2 (g) → MgO (aq) + SO2 (g) What will be the coefficient in front of O2 in the balanced chemical equation? If there is no coefficient in front of O2 in the balanced equation, please enter 1 as the answer.
For the following unbalanced reaction, suppose exactly 5.85 g of each reactant is taken. Determine which reactant is limiting, and also determine what mass of the excess reagent will remain after the limiting reactant is consumed. NaCl(s) + H₂SO4 (1) → HCl(g) + Na2SO4(s) Limiting reactant: Mass of excess reagent = g
For the following reaction, 0.358 moles of sulfuric acid are mixed with 0.228 moles of zinc hydroxide. sulfuric acid(aq) + zinc hydroxide(s) → zinc sulfate(aq) + water(e) What is the formula for the limiting reagent? What is the maximum amount of zinc sulfate that can be produced? moles
For each of the following balanced chemical equations, calculate how many moles and howmany grams of each product would be produced by the complete conversion of 0.50 mole ofthe reactant indicated in boldface. State clearly the mole ratio used for each conversion. NH 3 ‍ ( g ) + HCl ‍ ( g ) → NH 4 ‍ Cl ‍ ( s )