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Chapter 3: Problem 86

If \(1.5 \mathrm{~mol} \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}, 1.5 \mathrm{~mol} \mathrm{C}_{3} \mathrm{H}_{8},\) and \(1.5 \mathrm{~mol} \mathrm{CH}_{3} \mathrm{CH}_{2}\) \(\mathrm{COCH}_{3}\) are completely combusted in oxygen, which produces the largest number of moles of \(\mathrm{H}_{2} \mathrm{O} ?\) Which produces the least? Explain.

Short Answer

Expert verified
The compound which produces the largest number of moles of water when 1.5 moles are combusted is propane (C3H8) with 6.0 moles of H2O. Both ethanol (C2H5OH) and acetone (CH3CH2COCH3) produce the least number of moles of water with 4.5 moles of H2O each.

Step by step solution

01

Write down the combustion reactions

The combustion reactions of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}, \mathrm{C}_{3} \mathrm{H}_{8},\) and \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COCH}_{3}\) are as follows: Ethanol (C2H5OH) combustion: \[\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH} + 3 \mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2} + 3 \mathrm{H}_{2} \mathrm{O}\] Propane (C3H8) combustion: \[\mathrm{C}_{3} \mathrm{H}_{8} + 5 \mathrm{O}_{2} \rightarrow 3 \mathrm{CO}_{2} + 4 \mathrm{H}_{2} \mathrm{O}\] Acetone (CH3CH2COCH3) combustion: \[\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COCH}_{3} + 3.5 \mathrm{O}_{2} \rightarrow 3 \mathrm{CO}_{2} + 3 \mathrm{H}_{2} \mathrm{O}\]
02

Calculate the number of moles of water produced

For each compound, we will calculate the number of moles of water produced when 1.5 moles are combusted. 1.5 moles of ethanol combustion: \[1.5 \times \frac{3}{1} = 4.5 \mathrm{~moles~H}_{2} \mathrm{O}\] 1.5 moles of propane combustion: \[1.5 \times \frac{4}{1} = 6.0 \mathrm{~moles~H}_{2} \mathrm{O}\] 1.5 moles of acetone combustion: \[1.5 \times \frac{3}{1} = 4.5 \mathrm{~moles~H}_{2} \mathrm{O}\]
03

Compare the number of moles of water produced and draw conclusions

Based on the calculations above, the number of moles of water produced when 1.5 moles of each compound are combusted are: - Ethanol (C2H5OH): 4.5 moles of H2O - Propane (C3H8): 6.0 moles of H2O - Acetone (CH3CH2COCH3): 4.5 moles of H2O The compound which produces the largest number of moles of water is propane (C3H8), while ethanol (C2H5OH) and acetone (CH3CH2COCH3) both produce the least number of moles of water.

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Most popular questions from this chapter

Determine the formula weights of each of the following compounds: (a) nitrous oxide, \(\mathrm{N}_{2} \mathrm{O},\) known as laughing gas and used as an anesthetic in dentistry; (b) benzoic acid, \(\mathrm{HC}_{7} \mathrm{H}_{5} \mathrm{O}_{2}\), a substance used as a food preservative; (c) \(\mathrm{Mg}(\mathrm{OH})_{2}\), the active ingredient in milk of magnesia; (d) urea, \(\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}, \mathrm{a}\) compound used as a nitrogen fertilizer; (e) isopentyl acetate, \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{C}_{5} \mathrm{H}_{11}\), responsible for the odor of bananas.

A particular coal contains \(2.5 \%\) sulfur by mass. When this coal is burned at a power plant, the sulfur is converted into sulfur dioxide gas, which is a pollutant. To reduce sulfur dioxide emissions, calcium oxide (lime) is used. The sulfur dioxide reacts with calcium oxide to form solid calcium sulfite. (a) Write the balanced chemical equation for the reaction. (b) If the coal is burned in a power plant that uses 2000 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide? (c) How many grams of calcium sulfite are produced daily by this power plant?

(a) Define the terms limiting reactant and excess reactant. (b) Why are the amounts of products formed in a reaction determined only by the amount of the limiting reactant? (c) Why should you base your choice of which compound is the limiting reactant on its number of initial moles, not on its initial mass in grams?

The allowable concentration level of vinyl chloride, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl},\) in the atmosphere in a chemical plant is \(2.0 \times 10^{-6} \mathrm{~g} / \mathrm{L}\). How many moles of vinyl chloride in each liter does this represent? How many molecules per liter?

Aspirin \(\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\right)\) is produced from salicylic acid \(\left(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}\right)\) and acetic anhydride \(\left(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}\right):\) $$ \mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}+\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3} \longrightarrow \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}+\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2} $$ (a) How much salicylic acid is required to produce \(1.5 \times 10^{2} \mathrm{~kg}\) of aspirin, assuming that all of the salicylic acid is converted to aspirin? (b) How much salicylic acid would be required if only \(80 \%\) of the salicylic acid is converted to aspirin? (c) What is the theoretical yield of aspirin if \(185 \mathrm{~kg}\) of salicylic acid is allowed to react with \(125 \mathrm{~kg}\) of acetic anhydride? (d) If the situation described in part (c) produces \(182 \mathrm{~kg}\) of aspirin, what is the percentage yield?
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