Adipic acid, H.CeHsO4, used to produce nylon, is made commercially by a following reaction between cyclohexane (CsH12) and Oz: 2 CH12 + 5 O2 → 2 H2C&H&O4 + 2 H2O. Assume that you carry out this reaction with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. If you obtain 17.8 g of adipic acid, what is the percent yield for the reaction? Lütfen birini seçin: O a. 41.0% O b. 77.0% O c. 83.0% O d. 64.0% O e. 57.0%

Adipic acid, H.CeHsO4, used to produce nylon, is made commercially by a following reaction between cyclohexane (CsH12) and Oz: 2 CH12 + 5 O2 → 2 H2C&H&O4 + 2 H2O. Assume that you carry out this reaction with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. If you obtain 17.8 g of adipic acid, what is the percent yield for the reaction? Lütfen birini seçin: O a. 41.0% O b. 77.0% O c. 83.0% O d. 64.0% O e. 57.0%

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 47A

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Propane, C3H8, is the fuel of choice in a gas barbecue. When burning, the balanced equation is C3H8+5O23CO2+4H2O a What is the limiting reactant in cooking with a gas grill? b If the grill will not light and you know that you have an ample flow of propane to the burner, what is the limiting reactant? c When using a gas grill you can sometimes turn the gas up to the point at which the flame becomes yellow and smokey. In terms of the chemical reaction, what is happening?
4.69 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. 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.
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?
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.
Methanol, CH3OH, can be prepared from carbon monoxide and hydrogen. CO(g) + 2 H2(g) CH3OH(l) What mass of hydrogen is required to produce 1.0 L of CH3OH (d = 0.791 g/mL) if this reaction has a 74% yield under certain conditions?
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.
Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
Potassium chromate, a bright yellow solid, is produced by the reaction of solid chromium ore (FeCr2O4) with solid potassium carbonate and gaseous oxygen at high temperatures. The other products of the reaction are solid iron (III) oxide and gaseous carbon dioxide. If you use 169.0g of chromium ore, 298.0g of potassium carbonate and 75.00g of oxygen in a sealed reaction vessel, what is the limiting reagent? Give the theoretical yield of potassium chromate, in grams, for each one.
Cryolite (Na3AlF6) is used in the commercial production of aluminum from ore. Cryolite itself is produced by the following reaction: 6 NaOH + Al2O3 + 12 HF → 2 Na3AlF6 + 9 H2O A mixture containing 420.0 kg of NaOH, 128.4 kg of Al2O3, and 600.0 kg of HF is heated to 950 °C until it reacts to completion. What is the maximum mass of Na3AlF6 formed? ________kg Na3AlF6
Adipic acid, H2C6H8O4, used to produce nylon, is made commercially by a reaction between cyclohexane 1C6H122 and O2:2 C6H121l2 + 5 O21g2¡2 H2C6H8O41l2 + 2 H2O1g2(a) Assume that you carry out this reaction with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is thetheoretical yield of adipic acid? (b) If you obtain 33.5 g of adipic acid, what is the percent yield for the reaction?
Apidic acid (H2C6H8O4) is used to produce nylon. Apidic acid is made commercially by a reaction between cyclohexane (C6H12) and oxygen (O2). What is the balanced reaction for this transformation? (Hint: Water is formed as a by-product.) Assume that cyclohexane is the limiting reagent. You start with 25.0 g of cyclohexane. How much apidic acid could be produced? c. In reality, you only made 33.5 g of apidic acid. What is your % yield for the reaction?

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