Classify the following reactions as a combination, a combustion, or a decomposition reaction. Classify the following reactions as a combination, a combustion, or a decomposition reaction. Reaction 2 C2H2 (8)+502 (8)→ CO2 (g) + H2O (g) Reaction Type Answer 2 NH3 (g) + H2SO4 (aq) → (NH4)2SO4(aq) Answer ZnCO3 (s)→ ZnO (s) + CO2 (g) Answer 2 KMnO4(s)→K2MnO4 (s) + MnO2 (s) + O2(g) Answer SO3 (g) + H2O (e)→ H2SO4 (aq) Answer

Classify the following reactions as a combination, a combustion, or a decomposition reaction. Classify the following reactions as a combination, a combustion, or a decomposition reaction. Reaction 2 C2H2 (8)+502 (8)→ CO2 (g) + H2O (g) Reaction Type Answer 2 NH3 (g) + H2SO4 (aq) → (NH4)2SO4(aq) Answer ZnCO3 (s)→ ZnO (s) + CO2 (g) Answer 2 KMnO4(s)→K2MnO4 (s) + MnO2 (s) + O2(g) Answer SO3 (g) + H2O (e)→ H2SO4 (aq) Answer

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter4: Chemical Reactions

Section: Chapter Questions

Problem 4.72P

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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.
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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4.61 What is actually measured by the octane ratings of different grades of gasoline?
4.1 List at least two factors that make it difficult to describe the combustion of gasoline accurately. What assumption can be made to address these complications?
Acetone, (CH3)2CO, is an important industrial compound. Although its toxicity is relatively low, workers using it must be careful to avoid flames and sparks because this compound burns readily in air. Write the balanced equation for the combustion of acetone.
4-61 In photosynthesis, green plants convert CO2 and H2O to glucose, C6H12O6. How many grams of CO2are required to produce 5.1 g of glucose?
• describe the chemical processes used in biomass production and conversion to biofuels.
list at least three quantities that must be conserved in chemical reactions.
4-77 To convert 1 mol of iron(III) oxide to its elements requires 196.5 kcal: How many grams of iron can be produced if 156.0 kcal of heat is absorbed by a large-enough sample of iron(III) oxide?
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Oxidation of 1.00 g of carbon monoxide, CO, produces 1.57 g of carbon dioxide, CO2. How many grams of oxygen were required in this reaction?