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Chapter 3: Problem 88

If $2.0 \mathrm{~mol} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{COOH}, 2.0 \mathrm{~mol} \mathrm{C}_{4} \mathrm{H}_{10},\( and \)2.0 \mathrm{~mol}\( \)\mathrm{C}_{6} \mathrm{H}_{6}$ are completely combusted in oxygen, which one produces the largest number of moles of $\mathrm{H}_{2} \mathrm{O}$ ? Which one produces the least? Explain.

Short Answer

Expert verified
The compound that produces the largest number of moles of H₂O upon complete combustion is C₄H₁₀ (butane), with 10.0 moles of H₂O, while the compound that produces the least number of moles of H₂O is C₆H₆ (benzene), with 6.0 moles of H₂O.

Step by step solution

01

Write balanced chemical equations for the combustion reactions

For each compound, we can write a general equation for its combustion reaction: Compound + O₂ → CO₂ + H₂O Then, we balance the equations: 1. For the combustion of CH₃CH₂CH₂COOH (butanoic acid): \( C_4H_8O_2 + O_2 \rightarrow CO_2 + H_2O \) Balancing this equation, we get: \( C_4H_8O_2 + 6O_2 \rightarrow 4CO_2 + 4H_2O \) 2. For the combustion of C₄H₁₀ (butane): \( C_4H_{10} + O_2 \rightarrow CO_2 + H_2O \) Balancing this equation, we get: \( 2C_4H_{10} + 13O_2 \rightarrow 8CO_2 + 10H_2O \) 3. For the combustion of C₆H₆ (benzene): \( C_6H_6 + O_₂ \rightarrow CO₂ + H₂O \) Balancing this equation, we get: \( 2C_6H_6 + 15O_2 \rightarrow 12CO_2 + 6H_2O \)
02

Determine moles of H₂O produced by each compound

Now, for each combustion reaction equation, we calculate the number of moles of H₂O produced: 1. For the combustion of 2.0 moles of CH₃CH₂CH₂COOH: \( 2.0\,\text{mol}\,C_4H_8O_2 \times \frac{4\,\text{mol}\,H_2O}{1\,\text{mol}\,C_4H_8O_2} = 8.0\,\text{mol}\,H_2O \) 2. For the combustion of 2.0 moles of C₄H₁₀: \( 2.0\,\text{mol}\,C_4H_{10} \times \frac{10\,\text{mol}\,H_2O}{2\,\text{mol}\,C_4H_{10}} = 10.0\,\text{mol}\,H_2O \) 3. For the combustion of 2.0 moles of C₆H₆: \( 2.0\,\text{mol}\,C_6H_6 \times \frac{6\,\text{mol}\,H_2O}{2\,\text{mol}\,C_6H_6} = 6.0\,\text{mol}\,H_2O \)
03

Compare moles of H₂O to find the largest and smallest producers

The number of moles of H₂O produced in each case are: - For CH₃CH₂CH₂COOH: 8.0 moles of H₂O - For C₄H₁₀: 10.0 moles of H₂O - For C₆H₆: 6.0 moles of H₂O Therefore, the compound that produces the largest number of moles of H₂O is C₄H₁₀ (butane), and the compound that produces the least number of moles of H₂O is C₆H₆ (benzene).

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Most popular questions from this chapter

(a) Write "true" or "false" for each statement. (a) A mole of ducks contain a mole of feathers. (b) A mole of ammonia gas has a mass of \(17.0 \mathrm{~g}\). (c) The mass of 1 ammonia molecule is \(17.0 \mathrm{~g} .\) (d) \(\mathrm{A}\) mole of \(\mathrm{MgSO}_{4}(s)\) contains 4 moles of oxygen atoms.

Very small semiconductor crystals, composed of approximately 1000 to 10,000 atoms, are called quantum dots. Quantum dots made of the semiconductor CdSe are now being used in electronic reader and tablet displays because they emit light efficiently and in multiple colors, depending on dot size. The density of CdSe is \(5.82 \mathrm{~g} / \mathrm{cm}^{3}\) (a) What is the mass of one \(2.5-\mathrm{nm}\) CdSe quantum dot? (b) CdSe quantum dots that are \(2.5 \mathrm{nm}\) in diameter emit blue light upon stimulation. Assuming that the dot is a perfect sphere and that the empty space in the dot can be neglected, calculate how many Cd atoms are in one quantum dot of this size. (c) What is the mass of one \(6.5-\mathrm{nm}\) CdSe quantum dot? (d) CdSe quantum dots that are \(6.5 \mathrm{nm}\) in diameter emit red light upon stimulation. Assuming that the dot is a perfect sphere, calculate how many Cd atoms are in one quantum dot of this size. (e) If you wanted to make one \(6.5-\mathrm{nm}\) dot from multiple \(2.5-\mathrm{nm}\) dots, how many \(2.5-\mathrm{nm}\) dots would you need, and how many CdSe formula units would be left over, if any?

The molecular formula of saccharin, an artificial sweetener, is \(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{~S} .(\mathbf{a})\) What is the molar mass of saccharin? (b) How many moles of sachharin are in $2.00 \mathrm{mg}\( of this substance? (c) How many molecules are in \)2.00 \mathrm{mg}\( of this substance? (d) How many C atoms are present in \)2.00 \mathrm{mg}$ of saccharin?

Calculate the percentage by mass of oxygen in the following compounds: (a) vanillin, \(\mathrm{C}_{8} \mathrm{H}_{8} \mathrm{O}_{3} ;(\mathbf{b})\) isopropyl alcohol, \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}\); (c) acetaminophen, \(\mathrm{C}_{8} \mathrm{H}_{9} \mathrm{NO}_{2} ;\) (d) cyclopropanone, \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}\); (e) dioxin, \(\mathrm{C}_{12} \mathrm{H}_{4} \mathrm{Cl}_{4} \mathrm{O}_{2} ;\) (f) penicillin, $\mathrm{C}_{16} \mathrm{H}_{18} \mathrm{~N}_{2} \mathrm{O}_{4} \mathrm{~S}$.

Write balanced chemical equations for \((\mathbf{a})\) the complete combustion of acetone \(\left(\mathrm{CH}_{3} \mathrm{COCH}_{3}\right),\) a common organic solvent; (b) the decomposition of solid mercury (I) carbonate into carbon dioxide gas, mercury, and solid mercury oxide; (c) the combination reaction between sulphur dioxide gas and liquid water to produce sulfurous acid.
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