Example 3: The reaction that produces sugar in plants can be seen by the equation below. 3.6 mol of carbon dioxide reacts with 6.0 mol of water. What is the percentage yield of oxygen if only 72 g are recovered

Example 3: The reaction that produces sugar in plants can be seen by the equation below. 3.6 mol of carbon dioxide reacts with 6.0 mol of water. What is the percentage yield of oxygen if only 72 g are recovered

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

Determine percent yield for the reaction. 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(�)+O2(�)→2MgO(�) When 10.1 g of Mg are allowed to react with 10.5 g of O2, 11.6 g of MgO are collected.
A student knows the mass of one of the reactants of a chemical reaction and wants to calculate the mass of one of the products of the reaction. Which process should the student follow? Multiply the mass of the reactant by its molar mass to find the number of moles of the reactant. Use the chemical equation to find the number of moles of the product. Multiply the number of moles of the product by its molar mass to find the mass of the product. Multiply the mass of the reactant by its molar mass to find the number of moles of the reactant. Use the chemical equation to find the number of moles of the product. Divide the number of moles of the product by its molar mass to find the mass of the product. Divide the mass of the reactant by its molar mass to find the number of moles of the reactant. Use the chemical equation to find the number of moles of the product. Multiply the number of moles of the product by its molar mass to find the mass of the product. Divide the mass of the reactant…
For the following reaction, 62.6 grams of iron(III) oxide are allowed to react with 25.4 grams of aluminum.iron(III) oxide (s) + aluminum (s) aluminum oxide (s) + iron (s)What is the maximum amount of aluminum oxide that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams
Stoichiometry Review 1. Ammonium sulfate is used as a source of nitrogen in some fertilizers. It reacts with sodium hydroxide to produce sodium sulfate, water and ammonia, NH3. What mass of sodium hydroxide is required to react completely with 15.4 g of ammonium sulfate? 2. Iron (III) oxide, rust, can be removed from iron by reacting it with hydrochloric acid, HCl, to produce iron (III) chloride and water. What mass of hydrogen chloride is required to react with 100 of rust? 3. Dinitrogen pentoxide is a white solid. When heated it decomposes to produce nitrogen dioxide and oxygen. How many grams of oxygen gas will be produced in this reaction when 2.34 g of NO2 are made?
Part A Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 15.0 g of Fe203. MgO(s) + Fe(s) → Fe,O3(s) + Mg(s)
For the following reaction, 5.68 grams of chlorine gas are mixed with excess phosphorus (P4) . The reaction yields 5.34 grams of phosphorus trichloride .phosphorus (P4) ( s ) + chlorine ( g ) phosphorus trichloride ( l ) What is the theoretical yield of phosphorus trichloride ? grams What is the percent yield for this reaction ? %
Consider the balanced chemical equation: 3 H₂(g) + N₂(g) → 2 NH₃(g) If 46.8 g H₂ and 179.4 g N₂ are mixed to form NH₃, which of the following substances is the limiting reactant? A) nitrogen (N₂) B) hydrogen (H₂) C) ammonia (NH₃)
2. Ethyl chloride is prepared by the reaction of chlorine with ethane according to the following equation: C:Ho(g) + Cl2(g) – CH$CI(g) + HCl(g) Ethane Ethyl chloride a) Write the balanced chemical equation. Show proof of completion. b) When 5.6 g of ethane is reacted with excess chlorine, determine its theoretical yield c) Calculate the percent yield of ethyl chloride if experimental results indicated that 8.54 g of ethyl chloride had formed.
1. In a reaction of phosphorus and chlorine, both species is 25.0 g, which of the following assumption will be considered so P4 is the limiting reactant? a. Cl2’s mass must be lesser than the molar mass of P4. b.Cl2 must be greater than 25.0 g. c. Cl2 must be less than 25.0 g. d. Cl2’s mass must be greater than the molar mass of P4. e. Cl2 should be greater than 25.0 g 2.Which of the following approaches cannot be employed in doing the stoichiometry of gases? a.The approaches in solving gas stoic can be done on both reversible and irreversible. b.Differences in physical dimensions of variables may not be considered. c. Stoichiometry of gases can be proceeded regardless of quantity known. d. Gases should be taken differently due to physical conditions. e. Use the conservation of matter the same as solid and liquid. 3. Bleaching products contain sodium hypochlorite, a chlorine bleach. If you are the manufacturer of the bleach, how will you consider the amount of the…
For the following reaction, 24.7 grams of carbon disulfide are allowed to react with 95.8 grams of chlorine gas . carbon disulfide (s) + chlorine (g) – carbon tetrachloride (1) + sulfur dichloride (s) What he maximum amount of carbon tetrachloride that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams
Balance the chemical equation for the reaction of BaCl2 and Na2SO4 chemcial equation Using the balanced chemical equation, determine how many moles of NaCl will be produced, if 0.169 mol of BaCl2 is allowed to react with an excess of Na2SO4? moles of NaCl: Using the moles of NaCl found in the previous question, determine how many grams of NaCL can be produced. mass of NaCl: Using the moles of NaCl found in a previous question, determine how many formula units of NaCl can be produced. formula units:
Consider the following balanced chemical equation: 2NH3(g) + 5F2(g) → N2F4(g) + 6HF(g) Determine the theoretical yield of HF, in grams, when 54.60 g of NH3 reacts with 54.60 g of F2. g HF What is the percent yield if 7.180 g hydrogen fluoride (HF) is actually formed during the reaction?