When yeast is added to a solution of glucose or fructose, the sugars are said to undergo fermentation and ethyl alcohol is produced.СоН12О6 (аg) — 2C2H; ОН(ад) + 2C02(9)This is the reaction by which wines are produced from grape juice. Calculate the mass of ethyl alcohol, C2 H; OH, produced when 5.10 g of glucose, C6 H12 O6, undergoes thisreaction.g C2 H; OH

When yeast is added to a solution of glucose or fructose, the sugars are said to undergo fermentation and ethyl alcohol is produced. C6H12O6 (aq) → 2C2H5 OH(aq) + 2CO2(g) This is the reaction by which wines are produced from grape juice. Calculate the mass of ethyl alcohol, C2H; OH, produced when 5.10 g of glucose, C6H12O6 , undergoes this reaction. g C2H;OH

When yeast is added to a solution of glucose or fructose, the sugars are said to undergo fermentation and ethyl alcohol is produced. C6H12O6 (aq) → 2C2H5 OH(aq) + 2CO2(g) This is the reaction by which wines are produced from grape juice. Calculate the mass of ethyl alcohol, C2H; OH, produced when 5.10 g of glucose, C6H12O6 , undergoes this reaction. g C2H;OH

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 49A

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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.
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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.
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.
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3.100 Some aluminum—lithium alloys display the property of superplasticity, meaning they can undergo tensile deformation by large amounts (1000 times or more) without breaking. If such an alloy has 4 wt% Li, what is its composition in mol%? Explain the relative magnitudes of the mole percentage and weight percentage based on the molar masses of aluminum and lithium.
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
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4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g)+3H2O(l)3CO(g)+7H2(g)
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