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Chapter 5: Problem 24

Avogadro's number, molar mass, and the chemical formula of a compound are three useful conversion factors. What unit conversions can be accomplished using these conversion factors?

Short Answer

Expert verified
Using Avogadro's number, molar mass, and the chemical formula of a compound as conversion factors, we can accomplish the following unit conversions: 1. Convert the number of particles (atoms, molecules, ions, or electrons) to moles and vice versa using Avogadro's number. 2. Convert mass to moles and vice versa using molar mass. 3. Convert moles of one substance to moles of another substance, and moles of a substance to mass and vice versa using chemical formula and molar mass.

Step by step solution

01

Avogadro's number is a constant and represents the number of particles (atoms, molecules, ions, or electrons) in one mole of a substance. It is equal to approximately 6.022 x 10^23 particles per mole. Using Avogadro's number, we can convert between the number of particles and the amount of substance in moles. #Step 2: Unit conversions using Avogadro's Number#

With Avogadro's number, we can accomplish the following unit conversions: 1. Convert the number of particles (atoms, molecules, ions, or electrons) to moles: Divide the given number of particles by Avogadro's number. 2. Convert moles to the number of particles: Multiply the given number of moles by Avogadro's number. #Step 3: Understanding Molar Mass#
02

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole (g/mol). It can be calculated by adding up the atomic masses of all the atoms in a molecule or formula unit of a substance. Molar mass helps us convert between the mass of a substance and the amount of substance in moles. #Step 4: Unit conversions using Molar Mass#

With molar mass, we can accomplish the following unit conversions: 1. Convert mass to moles: Divide the given mass of a substance by its molar mass. 2. Convert moles to mass: Multiply the given number of moles by the molar mass of the substance. #Step 5: Understanding Chemical Formula#
03

The chemical formula of a compound tells us the type and number of each atom present in the compound. It can be used as a conversion factor to relate the moles of different atoms or compounds in a chemical reaction. #Step 6: Unit conversions using Chemical Formula#

With the chemical formula, we can accomplish the following unit conversions: 1. Convert moles of one substance to moles of another substance: Use the stoichiometric coefficients (numbers) in the balanced chemical equation. 2. Convert moles of a substance to mass and vice versa: Use the molar mass of the substance. In summary, the unit conversions that can be accomplished using Avogadro's number, molar mass, and the chemical formula are: - Number of particles to moles and vice versa - Mass to moles and vice versa - Moles of one substance to moles of another substance - Moles of a substance to mass and vice versa.

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Most popular questions from this chapter

An iron ore sample contains \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) plus other impurities. \(\mathrm{A}\) \(752-\mathrm{g}\) sample of impure iron ore is heated with excess carbon, producing \(453 \mathrm{g}\) of pure iron by the following reaction: $$\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{C}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}(g)$$ What is the mass percent of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) in the impure iron ore sample? Assume that \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) is the only source of iron and that the reaction is \(100 \%\) efficient.

Determine the molecular formulas to which the following empirical formulas and molar masses pertain. a. SNH (188.35 g/mol) c. \(\mathrm{CoC}_{4} \mathrm{O}_{4}(341.94 \mathrm{g} / \mathrm{mol})\) b. \(\mathrm{NPCl}_{2}(347.64 \mathrm{g} / \mathrm{mol})\) d. \(\mathrm{SN}(184.32 \mathrm{g} / \mathrm{mol})\)

In the production of printed circuit boards for the electronics industry, a 0.60-mm layer of copper is laminated onto an insulating plastic board. Next, a circuit pattern made of a chemically resistant polymer is printed on the board. The unwanted copper is removed by chemical etching, and the protective polymer is finally removed by solvents. One etching reaction is $$\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}(a q)+4 \mathrm{NH}_{3}(a q)+\mathrm{Cu}(s) \longrightarrow 2 \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}(a q)$$ A plant needs to manufacture 10,000 printed circuit boards, each \(8.0 \times 16.0 \mathrm{cm}\) in area. An average of \(80 . \%\) of the copper is removed from each board (density of copper \(=8.96 \mathrm{g} / \mathrm{cm}^{3}\)). What masses of \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\) and \(\mathrm{NH}_{3}\) are needed to do this? Assume \(100 \%\) yield.

A compound with molar mass \(180.1 \mathrm{g} / \mathrm{mol}\) has the following composition by mass: $$\begin{array}{|ll|}\hline C & 40.0 \% \\\H & 6.70 \% \\\O & 53.3 \% \\\\\hline\end{array}$$ Determine the empirical and molecular formulas of the compound.

Aspirin \(\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\right)\) is synthesized by reacting salicylic acid \(\left(\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}\right)\) with acetic anhydride \(\left(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}\right) .\) The balanced equation is $$\mathrm{C}_{7} \mathrm{H}_{6} \mathrm{O}_{3}+\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3} \longrightarrow \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}+\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}$$ a. What mass of acetic anhydride is needed to completely consume \(1.00 \times 10^{2}\) g salicylic acid? b. What is the maximum mass of aspirin (the theoretical yield) that could be produced in this reaction?
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