Q9) The equation for the complete combustion of methylpropane is 2CH3CH(CH3)CH3(g) + 1302(g) → 8CO₂(g) + 10H₂O(1) What amount, in mol, of carbon dioxide will be formed when three moles of methylpropane are combusted completely? C) 8 A) 12 B) 4 D) 16 E) Nome of them diavido CO2) in a sample of

Q9) The equation for the complete combustion of methylpropane is 2CH3CH(CH3)CH3(g) + 1302(g) → 8CO₂(g) + 10H₂O(1) What amount, in mol, of carbon dioxide will be formed when three moles of methylpropane are combusted completely? C) 8 A) 12 B) 4 D) 16 E) Nome of them diavido CO2) in a sample of

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.4PAE: 4.4 Automobile exhaust often contains traces of formaldehyde (CH2O), which is another possible...

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Question

Q9) The equation for the complete combustion of methylpropane is
2CH3CH(CH3)CH3(g) + 1302(g) → 8CO₂(g) + 10H₂O(1)
What amount, in mol, of carbon dioxide will be formed when three moles of
methylpropane are combusted completely?
C) 8
A) 12
B) 4
D) 16
E) Nome of them
diavido
CO2) in a sample of

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Heptane, C7H16, can be catalytically reformed to make toluene, C6H5CH3, another seven-carbon molecule. How many hydrogen molecules are produced for every toluene molecule derived from heptane? Write a balanced chemical equation for this reaction. Why is it profitable to convert heptane into toluene?
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?
How many carbon monoxide molecules (CO) are needed to react with 8 hydrogen molecules (H2) to produce methyl alcohol molecules (CH3OH)?
4.4 Automobile exhaust often contains traces of formaldehyde (CH2O), which is another possible product of incomplete combustion. Write a balanced equation for the formation of formaldehyde during the combustion of octane. (Water will also be formed as a product.)
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.
• describe the chemical processes used in biomass production and conversion to biofuels.
4.60 Why are fuel additives used?
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.
Choose the reaction that represents the combustion of C6H1202. C6H12O2(1) + 8 O2(g) →6 CO2(g) + 6 H₂O(g) O Mg(s) + C6H1202(1)→ MgC6H₁202(aq) 6 C(s) + 6 H₂(g) + O2(g) → C6H12O2(1) C6H12O2(1)→6 C(s) + 6 H₂(g) + O2(g) None of these represent the combustion of C6H12O2.
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