When powdered zinc is heated with sulfur, a violent reaction occurs, and zinc sulfide forms: Zn(s) S(s) - ZnS (s) [unbalanced] Some of the reactants also combine with oxygen in air to form zinc oxide and sulfur dioxide. When 83.2 g of Zn reacts with 52.4 g of Sg, 98.63 g of ZnS forms. Part 1 of 3 What is the percent yield of ZnS? Be sure your answer has the correct number of significant figures. % Part 2 of 3 If all the remaining reactants combine with oxygen, how many grams of ZnO form? Be sure your answer has the correct number of significant figures. g Part 3 of 3 X If all the remaining reactants combine with oxygen, how many grams of SO2 form? Be sure your answer has the correct number of significant figures. g 10

When powdered zinc is heated with sulfur, a violent reaction occurs, and zinc sulfide forms: Zn(s) S(s) - ZnS (s) [unbalanced] Some of the reactants also combine with oxygen in air to form zinc oxide and sulfur dioxide. When 83.2 g of Zn reacts with 52.4 g of Sg, 98.63 g of ZnS forms. Part 1 of 3 What is the percent yield of ZnS? Be sure your answer has the correct number of significant figures. % Part 2 of 3 If all the remaining reactants combine with oxygen, how many grams of ZnO form? Be sure your answer has the correct number of significant figures. g Part 3 of 3 X If all the remaining reactants combine with oxygen, how many grams of SO2 form? Be sure your answer has the correct number of significant figures. g 10

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 12CR: What is meant by a limiting reactant in a particular reaction? In what way is the reaction...

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Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?
In an experiment designed to produce calcium oxide by the chemical reaction 2Ca + O2 2CaO 177.2 g of CaO was obtained out of a possible 203.9 g ofCaO. a. What is the theoretical yield of CaO? b. What is the actual yield of CaO? c. What is the percent yield of CaO?
Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is HCl. Outline the steps needed to determine the percent yield of a reaction that produces 12.5 g of CCl2F2 from 32.9 g of Cd4. Freon-12 has been banned and is no longer used as a refrigerant because it catalyzes the decomposition of ozone and has a very long lifetime in the atmosphere. Determine the percent yield.
4-62 Iron ore is converted to iron by heating it with coal (carbon), and oxygen according to the following equation: If the process is run until 3940. g of Fe is produced, how many grams of CO2 will also be produced?
4.12 In petroleum refining, hydrocarbons are often manipulated by reacting them with H2(g). If hexene, C6H12, is reacted with hydrogen to form hexane, C6H14, how many moles of hydrogen are needed to react with 453 moles of hexene?
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
In Example 4.2, you found that a particular mixture of CO and H2 could produce 407 g CH3OH. CO(g) + 2H2(g) CH3OH (l) If only 332 g of CH3OH is actually produced, what is the percent yield of the compound?
When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
Calcium carbonate forms carbon dioxide and calcium oxide when it is heated above 900 °C in a limekiln. When heated to 1000 °C in a laboratory, 4.31 g calcium carbonate produces 2.40 g calcium oxide and 1.90 g carbon dioxide. Outline a method similar to combustion analysis by which you could determine the empirical formula for calcium carbonate from these data. Carry out the determination.
Methane (CH4) is the main component of marsh gas. Heating methane in the presence of sulfur produces carbon disulfide and hydrogen sulfide as the only products. a. Write the balanced chemical equation for the reaction of methane and sulfur. b. Calculate the theoretical yield of carbon disulfide when 120. g of methane is reacted with an equal mass of sulfur.

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