2 FeClz + 3 Zn à 3 ZnCl, + 2 Fe How many moles of Iron are produced when 0.75 moles of Zinc react with excess FeCl;? 55.847 65.39 35.453 Fe Zn CI 26 30 17 Iron Zinc Chlorine 2 FeClz + 3 Zn à 3 ZNCI, + 2 Fe How many grams of Iron are produced when 1.25 moles of Zinc react with excess FeCl;? 2 FeCl; + 3 Zn à 3 ZnCl, + 2 Fe How many grams of Iron are produced when 1.5g of Zinc react with excess FeCl, ? 63.546 35.453 26.98154 Cu CI AI 29 17 13 Copper Chlorine Aluminum 2A1 + 3CuCl, à 3Cu + 2A1C13 How many grams of Copper are produced when 1.5g of Aluminum react with excess CuCl,?

2 FeClz + 3 Zn à 3 ZnCl, + 2 Fe How many moles of Iron are produced when 0.75 moles of Zinc react with excess FeCl;? 55.847 65.39 35.453 Fe Zn CI 26 30 17 Iron Zinc Chlorine 2 FeClz + 3 Zn à 3 ZNCI, + 2 Fe How many grams of Iron are produced when 1.25 moles of Zinc react with excess FeCl;? 2 FeCl; + 3 Zn à 3 ZnCl, + 2 Fe How many grams of Iron are produced when 1.5g of Zinc react with excess FeCl, ? 63.546 35.453 26.98154 Cu CI AI 29 17 13 Copper Chlorine Aluminum 2A1 + 3CuCl, à 3Cu + 2A1C13 How many grams of Copper are produced when 1.5g of Aluminum react with excess CuCl,?

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 83AP

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Similar questions

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.
4.43 Magnesium nitride forms in a side reaction when magnesium metal burns in air. This reaction may also be carried out in pure nitrogen. 3Mg(s)+N2(g)Mg3N2(s) If 18.4 g of Mg3N2forms from the reaction of 20.0 g of magnesium with excess nitrogen, what is the percentage yield?
Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
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.
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4.47 Silicon carbide is, an abrasive used in the manufacture of grinding wheels. A company is investigating whether they can be more efficient in the construction of such wheels by making their own SiC via the reaction SiO2+3CSiC+2CO (a) If this reaction consistently has a yield of 85%, what is the minimum amount of both silicon dioxide and carbon needed to produce 3400 kg of SiC for the manufacture of cutting wheels? (b) The silicon dioxide is to he obtained from sand and the carbon is derived from coal. If the available sand is 95% SiO2 by weight and the coal is 73% C by weight, what mass of coal is needed for each metric ton of sand used?
3.93 Adipic acid is used in the production of nylon, so it is manufactured in large quantities. The most common method for the preparation of adipic acid is the reaction of cyclohexane with oxygen. Balance the skeleton equation shown be1ow.
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