4. 2.00 g of Zn metal reacts with 2.50 g silver nitrate to produce silver metal and zinc nitrate. 1) What reactant is limiting? 2) How many grams of Ag and zinc nitrate are formed? What mass of the excess reagent is left after the reaction? 3) How to calculate Percent Yield? Silicon carbide (SiC) is an important ceramic material that is made by allowing sand (silicon dioxide, 5. SiO2) to react with powdered carbon at high temperature. Carbon monoxide is also formed. When 100.0 g of sand is processed, 51.4 g of SiC is recovered. What is the percent yield of SiC from this process?

4. 2.00 g of Zn metal reacts with 2.50 g silver nitrate to produce silver metal and zinc nitrate. 1) What reactant is limiting? 2) How many grams of Ag and zinc nitrate are formed? What mass of the excess reagent is left after the reaction? 3) How to calculate Percent Yield? Silicon carbide (SiC) is an important ceramic material that is made by allowing sand (silicon dioxide, 5. SiO2) to react with powdered carbon at high temperature. Carbon monoxide is also formed. When 100.0 g of sand is processed, 51.4 g of SiC is recovered. What is the percent yield of SiC from this process?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter4: Stoichiometry Of Chemical Reactions

Section: Chapter Questions

Problem 65E: Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is...

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Chlorine and fluorine react to form gaseous chlorine trifluoride. Initially, 1.75 mol of chlorine and 3.68 mol of fluorine are combined. (Assume 100% yield for the reaction.) (a) Write a balanced equation for the reaction. (b) What is the limiting reactant? (c) What is the theoretical yield of chlorine trifluoride in moles? (d) How many moles of excess reactant remain after reaction is complete.
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.
Sodium metal reacts with molecular iodine to produce sodium iodide. If 10.0 moles of sodium reacts with 15.0 moles of iodine, (a) what is the limiting reagent, (b) the theoretical yield of sodium iodide in moles can be produced and (c) the amount in moles of the excess reagent remains after the completion of the reaction?
1. Oxygen bleach acts in the release of oxygen which best works in hot water mixture. Which of the following bleach or its derivative could be a potential for oxygen bleaching? -OCl- NaOH NaOCl -O²- H2O2 2. In the production of ceramic, silicon carbide and silicon dioxide are being reacted at high temperature. In the process, carbon monoxide is also produced. After the reaction of 100.0 kg of silicon dioxide, 51.4 kg of SiC is obtained. Determine the percent yield of silicon carbide.
a) Write a balanced reaction for the process of reacting potassium with oxygen to form potassium oxide, or K2O. ---> 4K + O2 -> 2K2O2b) Suppose 10.0g of potassium reacts with excess oxygen gas, and 10.5 g of K2O is produced. What is the percent yield?c) Now suppose 4.0g of potassium and 1.0g of oxygen gas react in a closed flask. How much K2O can be produced?d) Assuming 100% yield in part (c), how many grams of the excess reactant will be left over after the reaction is complete Please answer parts b - d (which is 3 parts)
When water is added to solid calcium carbide, CaC2, the produces are acetylene gas, C2H2, and aqueous calcium hydroxide.a. Write the balanced chemical equation for this reaction.b. How many moles of acetylene are produced when 0.50 moles of calcium carbide react?c. How many moles of calcium carbide are needed to completely react with 5.00x1022 water molecules?
Coal Combustion -- Limestone for SO2 Scrubbing Limestone(CaCO3) is used to remove acidic pollutants from smokestack flue gases in a sequence of decomposition-combination reactions. The limestone is heated to form lime (CaO), which reacts with sulfur dioxide to form calcium sulfite. Assuming a 70.5% yield in the overall reaction, what mass of limestone is required to remove all the sulfur dioxide formed by the combustion of 69000 kg coal that is 0.42 mass % sulfur?
When a mixture of 10.0 g of acetylene 1C2H22 and 10.0 g ofoxygen 1O22 is ignited, the resulting combustion reactionproduces CO2 and H2O. (a) Write the balanced chemicalequation for this reaction. (b) Which is the limiting reactant?(c) How many grams of C2H2, O2, CO2, and H2O arepresent after the reaction is complete?
The first step in the manufacture of nitric acid by the Ostwald process is the reaction of ammonia gas with oxygen, producing nitrogen oxide and steam. The reaction mixture contains 8.26 g of ammonia and 10.2 g of oxygen. After the reaction is complete, 6.67 g of nitrogen oxide are obtained. Write a balanced equation for the reaction. How many grams of nitrogen oxide can be theoretically obtained? How many grams of excess reactant are theoretically unused? What is the percent yield of the reaction? g nitric oxide g excess reactant %
gIVEN THE FOLLOWING EQUATION OF THE COMBUSTION OF BUTANE C4H10 + O2 ARROW CO2 + H2O A. WHICH IS THE LIMITING REACTANT IF THE REACTION STARTED WITH: 6 MOL OF C4H10 AND 8 MOL OF 02? B. WHAT IS THE PERCENTAGE ERROR IF THE ACTUAL YIELD IS 4.5 MOL CO2? C. HOW MUCH IS THE LEFT OVER OF THE EXCESS REACTANT?
When 5.0g of Hydrogen is combined with 5.0g of Fluorine, which is the limiting reactant? florine or hydrogen
Ferric chloride, FeCl3 reacts with silver nitrate, AgNO3 to form ferric nitrate, Fe (NO3)3 and silver chloride, AgCl. a. Write the balanced chemical equation of the reaction. b. If 108.5 moles of FeCl3 is combined with 76.8 moles of AgNO3, how many moles of AgCl is produced? c. How many grams of AgCl is produced? d. Which reactant is the limiting reagent? e. Which reactant is the excess reagent?