When 46.19 g NH3 reacts by the following balanced equation, 27.98 H₂O are formed.4NH3(g) +502(g)4NO(g) +6H2O(g)(a) What is the theoretical yield of H₂O? (b) What is the percent yield of H₂O? Please include the conversionfactors (i.e. 1 mol - 28g CO) used in the calculation and show your math work to receive full credit.

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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...

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What is the limiting reactant when 10.0 g of carbon monoxide (CO, molar mass = 28.01 g∙mol–1) and 15.0 g of iron(III) oxide (Fe2O3, molar mass = 159.70 g∙mol–1) are allowed to react completely to form carbon dioxide (CO2) and iron (Fe). Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g)
For the following reaction, 4.25 grams of carbon disulfideare mixed with excess chlorine gas. Assume that the percent yield of carbon tetrachloride is 67.6 %.CS2 (s) + 4Cl2 (g) CCl4 (l) + 2SCl2 (s) (1) What is the theoretical yield of carbon tetrachloride (in grams)? (2) What is the actual yield of carbon tetrachloride (in grams)?
A chemist invents a new combustion analysis instrument that uses less O2(g) which saves money on each analysis. The improvement is that instead of CO2(g) being formed and trapped, CO(g) is formed and trapped. H2O (g) is also formed and trapped when substances that contain hydrogen are analyzed.(a) The chemist places 2.184 g of an unknown compound of carbon and hydrogen in the new analyzer. 4.627 g of CO (g) and 1.795 g of H2O (g) are produced. Find the empirical formula for the compound.(Molar masses (g/mol): CO = 28.0104, H2O = 18.015) (b) Despite the best efforts of the chemist, the molar mass of the compound cannot be determined (using this method). Clearly explain why this prevents the determination of the molecular formula
Consider the unbalanced equation for the combustion of hexane: αC6H14(g)+βO2(g)→γCO2(g)+δH2O(g) Determine how many moles of O2 are required to react completely with 7.4 mol of C6H14. Express your answer using two significant figures.
Use the References to access important values if needed for this question. For the following reaction. 5.63 grams of iron(III) oxide are mixed with excess aluminum. The reaction yields 2.88 grams of aluminum oxide. Fe₂O₂ (s) + 2Al(s) Al₂O, (s) 2Fe (s) (1) What is the theoretical yield of aluminum oxide? (2) What is the percent yield for this reaction? % grams
6. Consider the reaction: 4Al(s) + 3029) – > 2Al2O3(s) (a) If 9.00 moles of aluminum react with an excess of oxygen, how many moles of aluminum oxide are produced? (b) The production of 0.435 moles of aluminum oxide requires the reaction of moles of aluminum and (c) When 1.730 moles of aluminum reacts, moles of oxygen? moles of oxygen are consumed.
Glucose, C6H1206, can be represented by the molecular model shown below. If 1.00 mol of glucoseis submitted to combustion analysis, how many moles of CO2 and how many moles of H2O wouldbe formed?
Use the References to access important values if needed for this question. For the following reaction, 4.29 grams of oxygen gas are mixed with excess propane (C3Hg). The reaction yields 2.81 grams of carbon dioxide. (1) What is the theoretical yield of carbon dioxide? (2) What is the percent yield for this reaction? C3Hg (g) +50₂ (g) 3CO₂ (g) + 4H₂O(g) % grams
Dichlorine monoxide, Cl,0, is sometimes used as a powerful chlorinating agent in research. It can be produced by passing chlorine gas over heated mercury(I) oxide according to this equation: HgO+Cl2 → HgCl, + Cl20 What is the percent yield, if the quantity of reactants is sufficient to produce 8.90 g of Cl,0 but only 2.10 g is obtained? Answer in standard notation to the nearest tenth of a percent
Give a clear handwritten answer
4. The reaction for the combustion of propene is:2 C3H6 + 9O2 6 CO2 + 6 H2O(a) If 15.0 g of C3H6 and 15.0 g of O2 are reacted, how many moles of H2O can be produced?(b) If 12.0 g of C3H6 and 25.0 g of O2 are reacted, how many moles of H2O can be produced?(c) If 5.0 mol of C3H6 and 15.0 mol of O2 are reacted to completion (until one reactant is completely used up), how many moles of CO2 can be produced? Which reactant is left over when the reaction has gone to completionin a closed container?
3. When heated, lithium reacts with nitrogen to form lithium nitride: 6Li(s) + N₂(g) →→→ 2Li3N (s) (a) What is the theoretical yield of Li3N in grams when 12.3 g of Li are heated with 33.6 g of N₂? (b) If the actual yield of Li3N is 5.89 g, what is the percent yield of the reaction? 4. Calculate the molarity of each of the following solutions: (a) 29.0 g of ethanol (C₂H5OH) in 545 mL of solution (b) 15.4 g of sucrose (C12H22011) in 74.0 mL of solution

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