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Chapter 3: Problem 36

(a) What is the mass, in grams, of \(1.223 \mathrm{~mol}\) of iron(III) sulfate? (b) How many moles of ammonium ions are in \(6.955 \mathrm{~g}\) of ammonium carbonate? (c) What is the mass, in grams, of \(1.50 \times 10^{21}\) molecules of aspirin, \(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4} ?\) (d) What is the molar mass of diazepam (Valium \(^{\circ}\) ) if 0.05570 mol has a mass of \(15.86 \mathrm{~g}\) ?

Short Answer

Expert verified
(a) The mass of $1.223\, \text{mol}$ of iron(III) sulfate is \(\boldsymbol{399.95 \, \text{g}}\). (b) There are \(\boldsymbol{0.2688\, \text{mol}}\) of ammonium ions in $6.955\, \text{g}$ of ammonium carbonate. (c) The mass of $1.50 \times 10^{21}$ molecules of aspirin is \(\boldsymbol{6.009 \, \text{g}}\). (d) The molar mass of diazepam is \(\boldsymbol{284.8 \, \text{g/mol}}\).

Step by step solution

01

Find the molar mass of iron(III) sulfate

To find the mass of iron(III) sulfate, we first need to find its molar mass. Iron(III) sulfate has the chemical formula Fe2(SO4)3. It consists of two Fe atoms, three SO4 units, totaling nine O atoms and three S atoms. To calculate the molar mass of Iron(III) sulfate, multiply the number of atoms of each element by their atomic weights and sum them: \(Molar \, mass = 2 \times (molar \, mass \, of \, Fe) + 3 \times [4 \times (molar \, mass \, of \, O) + (molar \, mass \, of \, S)]\)
02

Calculate the mass of iron(III) sulfate

To calculate the mass of iron(III) sulfate, multiply the given moles by its molar mass: \( Mass = Moles \times Molar \, mass \) #Problem (b)#
03

Obtain the molar mass of ammonium carbonate and calculate moles

Ammonium carbonate has the formula (NH4)2CO3. To calculate the required moles of ammonium ions, first, we find the molar mass of ammonium carbonate and then find the moles of the compound: \( Moles = \frac{Mass}{Molar \, mass} \) Finally, we can determine the moles of ammonium ions in the given mass of ammonium carbonate. #Problem (c)#
04

Find the molar mass of aspirin

Aspirin has the chemical formula C9H8O4. To find the molar mass of aspirin, we multiply the number of atoms of each element by their atomic weights and sum them: \( Molar \, mass \, of \, aspirin = 9 \times (molar \, mass \, of \, C) + 8 \times (molar \, mass \, of \, H) + 4 \times (molar \, mass \, of \, O) \)
05

Calculate the number of moles and mass of aspirin

First, we need to determine the number of moles to calculate the mass of aspirin: \( Number \, of \, moles = \frac{Number \, of \, particles}{Avogadro's \, number}\) Once we have the number of moles, we can find the mass of aspirin using the following formula: \( Mass = Moles \times Molar \, mass \) #Problem (d)#
06

Calculate the molar mass of diazepam

For diazepam, we are given the mass and the number of moles. We can simply find the molar mass using the formula: \( Molar \, mass = \frac{Mass}{Moles} \)

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Most popular questions from this chapter

(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?

Determine the empirical and molecular formulas of each of the following substances: (a) Ibuprofen, a headache remedy, contains \(75.69 \% \mathrm{C}, 8.80 \%\) \(\mathrm{H},\) and \(15.51 \% \mathrm{O}\) by mass, and has a molar mass of \(206 \mathrm{~g} / \mathrm{mol}\) (b) Cadaverine, a foul-smelling substance produced by the action of bacteria on meat, contains \(58.55 \% \mathrm{C}, 13.81 \% \mathrm{H},\) and \(27.40 \% \mathrm{~N}\) by mass; its molar mass is \(102.2 \mathrm{~g} / \mathrm{mol}\). (c) Epinephrine (adrenaline), a hormone secreted into the bloodstream in times of danger or stress, contains \(59.0 \% \mathrm{C}\), \(7.1 \% \mathrm{H}, 26.2 \% \mathrm{O},\) and \(7.7 \% \mathrm{~N}\) by mass; its \(\mathrm{MW}\) is about 180 amu.

What parts of balanced chemical equations give information about the relative numbers of moles of reactants and products involved in a reaction?

Consider a sample of calcium carbonate in the form of a cube measuring 2.005 in. on each edge. If the sample has a density of \(2.71 \mathrm{~g} / \mathrm{cm}^{3},\) how many oxygen atoms does it contain?

Calculate the following quantities: (a) mass, in grams, of \(1.50 \times 10^{-2} \mathrm{~mol}\) of CdS (b) number of moles of \(\mathrm{NH}_{4} \mathrm{Cl}\) in \(86.6 \mathrm{~g}\) of this substance (c) number of molecules in \(8.447 \times 10^{-2} \mathrm{~mol} \mathrm{C}_{6} \mathrm{H}_{6}\) (d) number of \(\mathrm{O}\) atoms in \(6.25 \times 10^{-3} \mathrm{~mol} \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\)
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