© Macmillan LearningA sample of 92.0 g of tetraphosphorous decoxide (P4010) reacts with 49.9 g of water to produce phosphoric acid (H₂PO₂)according to the following balanced equation.P4010 + 6H₂O4 H₂PO4Determine the limiting reactant for the reaction.O H₂PO4O H₂OOP₂010Calculate the mass of H3PO4 produced in the reaction.mass of H₂PO4:Calculate the percent yield of H3PO4 if 46.9 g of H3PO4 is isolated after carrying out the reaction.percent yield:Search or type URL76MacBook ProY&N7U8+(9(0)0P+ 1183%6.0gde

Answered: Image /qna-images/answer/5adb5ac8-79ee-4e4a-b7a1-296c039fb9d0.jpg

Macmillan Learning A sample of 92.0 g of tetraphosphorous decoxide (P4010) reacts with 49.9 g of water to produce phosphoric acid (H₂PO4) according to the following balanced equation. P4010 + 6H₂O4 H₂PO4 Determine the limiting reactant for the reaction. OH₂PO4 OH₂O P4010 Calculate the mass of H3PO4 produced in the reaction. mass of H₂PO4: Calculate the percent yield of H3PO4 if 46.9 g of H₂PO4 is isolated after carrying out the reaction. percent yield: % g

Macmillan Learning A sample of 92.0 g of tetraphosphorous decoxide (P4010) reacts with 49.9 g of water to produce phosphoric acid (H₂PO4) according to the following balanced equation. P4010 + 6H₂O4 H₂PO4 Determine the limiting reactant for the reaction. OH₂PO4 OH₂O P4010 Calculate the mass of H3PO4 produced in the reaction. mass of H₂PO4: Calculate the percent yield of H3PO4 if 46.9 g of H₂PO4 is isolated after carrying out the reaction. percent yield: % g

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

K $ 4 R For the following reaction, 4.16 grams of hydrogen gas are allowed to react with 45.2 grams of iodine hydrogen (g) + iodine (s)→ hydrogen iodide (g) What is the maximum amount of hydrogen iodide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? Submit Answer % 5 [Review Topics] [References] Use the References to access important values if needed for this question. Show Hint T Retry Entire Group 4 more group attempts remaining Cengage Learning Cengage Technical Support < 6 Y d 7 U 8 I < ( 9 0 O P grams grams * Previous 4) [
How many grams of iron need to react to produce 91.4 g iron(III) oxide according to the balanced reaction below? 4 Fe (s) + 3O2 (g) 2 Fe2O3 (s)
The following equation represents the formation of nitrogen dioxide, a major component of smog,2 NO + O2 → 2 NO2 If 0.68 mole of NO is reacted with 0.79 mole of O2 to produce NO2, the limiting reactant is The following equation represents the formation of nitrogen dioxide, a major component of smog,2 NO + O2 → 2 NO2 If 0.68 mole of NO is reacted with 0.79 mole of O2 to produce NO2, the limiting reactant is both NO and O2. NO. NO2. O2. Interpret in words the equation shown.P4O10 (s) + 6 H2O (l) → 4 H3PO4 (aq) Interpret in words the equation shown.P4O10 (s) + 6 H2O (l) → 4 H3PO4 (aq) One mole of phosphorus(X) oxide combines with six moles of water to produce four moles of solution of hydrogen phosphate. Four moles of solid phosphorus, five moles of diatomic oxygen gas, and six moles of liquid water react together to produce four moles of phosphoric acid in solution. Four atoms of phosphorus, 16 atoms of oxygen, and 12 atoms of hydrogen rearrange to produce…
Follow the rules of significant digits. Balance the reaction below. How many moles of oxygen gas reacted if 5.32 moles of carbon dioxide were produced? C3H16 (g) + 02 (g) --> CO2 (g) + H20 (g)
consider the following balanced equation 15O2(g)+2C6H5COOH(aq) ___ 14CO2(g)+6H2O(I) if 11.6 moles of O2(g) and 2.34 moles of C6H5COOH(aq) are allowed to react, and the percent yield is 76.7% how many moles of H2O(I) will actually be produced?
How many grams of N2 are needed to completely (stoichiometrically) react with 222 g of Br2 ? N2 + 3 Br2 2 NB13 + 44.0 kJ The molar mass of Br2 is g and the molar mass of N2 is mol Br2 (2.22 x 102 g Br2)(- mol Br2 g Br2 mol N2 mol Br2 (-- -) = mol N2 mol Br2 g N2 mol N2 (-- -) = |v g N2 mol N2 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.38 х 100 h. 3.26 x 103 i. 44.0 j. 1.33 x 102 k. 9.77 x 103 I. 4.44 x 102 m. 6.66 x 10² n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved Cc. absorbed dd. exothermic ee. endothermic
22.0 g of CO2 gas and 9.01 g of H2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?
You have 22.2 g of the compound C2Hx, where x is the maximum number of hydrogens that can fit around two carbon atoms and still create a stable Lewis dot structure. If you allow all of this sample to react with excess oxygen and then allow the products to cool to room temperature, how many moles of liquid product will you have?
Given the following balanced chemical equation: 2 CO(g) + O2(g) 2CO2(g) 15.0 g of CO(g) and 15.0 g of O2(g) placed in this reaction a) Determine the limiting and excess reactant. Calculate the mass of product produced to support your answers. b) If 1.52 g of CO2(g) produced at the end of the reaction, what is the percent yield? actual yield Percent yield x 100 theoretical yield c) Calculate the mass of the excess reactant left over.
A sample of 48.7 g of tetraphosphorous decoxide (P₂O₁0) reacts with 84.6 g of water to produce phosphoric acid (H₂PO4) according to the following balanced equation. PAO10 + 6H₂O4 H₂PO4 Determine the limiting reactant for the reaction. OH₂O O H₂PO4 OP40 10 Calculate the mass of H₂PO4 produced in the reaction. mass of H₂PO4:
If 54.7 grams of propane (C3H8) and 89.6 grams of oxygen (O2) are available in the balanced combustion reaction below: C3H8 + 5 O2 -> 3 CO2 + 4 H2O Determine which reactant is the limiting