Q: Which calculation would you use to find the number of moles of ibuprofen that contain $2.00 \times 10^{24}$ atoms of carbon? (Ibuprofen formula: $\mathrm{C_{13}H_{18}O_2}$)

Divide $2.00 \times 10^{24}$ by Avogadro's number, then divide by 13.

Question 1

Ibuprofen has the molecular formula $\mathrm{C_{13}H_{18}O_2}$. What is the molar mass of ibuprofen?

Accepted Answer

$206\ \mathrm{g/mol}$

Question 2

How many grams of ibuprofen are present in $0.525$ mole? (Molar mass of ibuprofen $= 206\ \mathrm{g/mol}$)

Accepted Answer

$108.15\ \mathrm{g}$

Question 3

If you have $12.0\ \mathrm{g}$ of ibuprofen ($\mathrm{C_{13}H_{18}O_2}$), how many moles of carbon atoms are present?

Accepted Answer

$0.757\ \mathrm{mol}$

Question 4

How many moles of ibuprofen contain $1.22 	imes 10^{23}$ atoms of carbon? (Ibuprofen formula: $\mathrm{C_{13}H_{18}O_2}$)

Accepted Answer

$0.0151\ \mathrm{mol}$

Question 5

A patient is prescribed $400\ \mathrm{mg}$ of ibuprofen. How many moles of ibuprofen does this represent? (Molar mass $= 206\ \mathrm{g/mol}$)

Accepted Answer

$0.00194\ \mathrm{mol}$

Question 6

If a tablet contains $2.00 	imes 10^{21}$ molecules of ibuprofen, how many grams of ibuprofen are in the tablet? (Molar mass $= 206\ \mathrm{g/mol}$, Avogadro's number $= 6.022 	imes 10^{23}$)

Accepted Answer

$0.684\ \mathrm{mg}$

Question 7

Which of the following best describes the process to determine the number of moles of carbon atoms in a given mass of ibuprofen?

Accepted Answer

Divide the mass of ibuprofen by its molar mass, then multiply by 13.

Question 8

A pharmacist needs to prepare a solution containing $0.250\ \mathrm{mol}$ of ibuprofen. What mass of ibuprofen is required? (Molar mass $= 206\ \mathrm{g/mol}$)

Accepted Answer

$51.5\ \mathrm{g}$

Question 9

If a dose contains $3.00 	imes 10^{22}$ molecules of ibuprofen, how many moles of ibuprofen does this represent?

Accepted Answer

$0.0000498\ \mathrm{mol}$

Question 10

A sample contains $0.100\ \mathrm{mol}$ of ibuprofen. How many molecules of ibuprofen are present? (Avogadro's number $= 6.022 	imes 10^{23}$)

Accepted Answer

$6.02 	imes 10^{22}$

Question 11

Which calculation would you use to find the number of moles of ibuprofen that contain $2.00 	imes 10^{24}$ atoms of carbon? (Ibuprofen formula: $\mathrm{C_{13}H_{18}O_2}$)

Accepted Answer

Divide $2.00 	imes 10^{24}$ by Avogadro's number, then divide by 13.

Question 12

A patient accidentally takes $1.00\ \mathrm{g}$ of ibuprofen. How many molecules of ibuprofen did they ingest? (Molar mass $= 206\ \mathrm{g/mol}$, Avogadro's number $= 6.022 	imes 10^{23}$)

Accepted Answer

$2.92 	imes 10^{22}$

Question 13

If a chemist wants to isolate $1.00 	imes 10^{24}$ atoms of hydrogen from ibuprofen, how many moles of ibuprofen are needed? (Ibuprofen formula: $\mathrm{C_{13}H_{18}O_2}$)

Accepted Answer

$0.0925\ \mathrm{mol}$

Question 14

Which of the following best explains why the number of moles of carbon atoms in a sample of ibuprofen is greater than the number of moles of ibuprofen molecules?

Accepted Answer

Each molecule of ibuprofen contains more than one carbon atom.

Question 15

A solution contains $0.0500\ \mathrm{mol}$ of ibuprofen. How many atoms of oxygen are present in the solution? (Ibuprofen formula: $\mathrm{C_{13}H_{18}O_2}$, Avogadro's number $= 6.022 	imes 10^{23}$)

Accepted Answer

$1.20 	imes 10^{23}$

Mole Calculations and Molar Mass: Ibuprofen as a Case Study

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