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Chapter 3: Problem 29

(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.

Short Answer

Expert verified
False, True, False, True

Step by step solution

01

Statement (a)

A mole of ducks contain a mole of feathers. This statement is comparing the amount of ducks to the amount of feathers. In chemistry, a mole is defined as 6.022 x 10^23 representative particles of a substance, and it is a way of counting entities like atoms and molecules. Therefore, comparing the moles of ducks to moles of feathers is not correct. The correct answer for this statement is: False
02

Statement (b)

A mole of ammonia gas has a mass of 17.0 g. In order to find out whether this statement is true or false, we need to determine the molar mass of ammonia (NH3). We can find this by adding the molar masses of all the atoms in ammonia: - Nitrogen (N): \(14.01 \mathrm{~g/mol}\) - Hydrogen (H): \(1.01 \mathrm{~g/mol}\) So, the molar mass of ammonia (NH3) is: \((1\times 14.01) + (3\times 1.01) = 17.03 \mathrm{~g/mol}\) Since a mole of ammonia has a mass of 17.03 g, the statement is almost true, and we'll consider it as: True
03

Statement (c)

The mass of 1 ammonia molecule is 17.0 g. This statement is confusing the mass of 1 mole of ammonia (found in statement b) with the mass of a single ammonia molecule. Since we have already determined that a mole of ammonia has a mass of 17.03 g, we can find the mass of 1 ammonia molecule by dividing the mass of 1 mole of ammonia by Avogadro's number (6.022 x 10^23): Mass of 1 ammonia molecule = \(\frac{17.03 \mathrm{~g/mol}}{6.022 \times 10^{23} \mathrm{~molecules/mol}}\) The resulting mass of one ammonia molecule is much smaller than 17.0 g, so this statement is: False
04

Statement (d)

A mole of MgSO4 (s) contains 4 moles of oxygen atoms. To verify this statement, we need to look at the formula of magnesium sulfate (MgSO4) and count the number of oxygen atoms per formula unit. We see that there is one sulfur atom and four oxygen atoms bonded to it in the sulfate ion (SO4^2-), so in one formula unit of MgSO4, there are indeed 4 oxygen atoms. Therefore, 1 mole of MgSO4 contains 4 moles of oxygen atoms, and this statement is: True

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Most popular questions from this chapter

Balance the following equations: (a) $\mathrm{HClO}_{4}(a q)+\mathrm{P}_{4} \mathrm{O}_{10}(s) \longrightarrow \mathrm{HPO}_{3}(a q)+\mathrm{Cl}_{2} \mathrm{O}_{7}(l)$ (b) $\mathrm{Au}_{2} \mathrm{~S}_{3}(s)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{Au}(s)+\mathrm{H}_{2} \mathrm{~S}(g)$ (c) $\mathrm{Ba}_{3} \mathrm{~N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(a q) \longrightarrow \mathrm{Ba}(\mathrm{OH})_{2}(a q)+\mathrm{NH}_{3}(g)$ (d) $\mathrm{Na}_{2} \mathrm{CO}_{3}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g)$

(a) Ibuprofen is a common over-the-counter analgesic with the formula \(\mathrm{C}_{13} \mathrm{H}_{18} \mathrm{O}_{2} .\) How many moles of \(\mathrm{C}_{13} \mathrm{H}_{18} \mathrm{O}_{2}\) are in a 500-mg tablet of ibuprofen? Assume the tablet is composed entirely of ibuprofen. (b) How many molecules of $\mathrm{C}_{13} \mathrm{H}_{18} \mathrm{O}_{2}$ are in this tablet? (c) How many oxygen atoms are in the tablet?

Vanillin, the dominant flavoring in vanilla, contains C, H, and O. When $1.05 \mathrm{~g}\( of this substance is completely combusted, \)2.43 \mathrm{~g}$ of \(\mathrm{CO}_{2}\) and \(0.50 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) are produced. What is the empirical formula of vanillin?

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?

The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between sodium bicarbonate \(\left(\mathrm{NaHCO}_{3}\right)\) and citric acid $\left(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)$ $$ \begin{aligned} 3 \mathrm{NaHCO}_{3}(a q)+\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}(a q) & \longrightarrow \\ 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Na}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}(a q) \end{aligned} $$ In a certain experiment \(1.00 \mathrm{~g}\) of sodium bicarbonate and $1.00 \mathrm{~g}$ of citric acid are allowed to react. (a) Which is the limiting reactant? (b) How many grams of carbon dioxide form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?
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