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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