QuestionJune 17, 2025

A typical dose of loperamide for an adult is 4.0 mg. What mass of carbon atoms is there in a 4.0 mg dose of loperamide? (1 Point)

A typical dose of loperamide for an adult is 4.0 mg. What mass of carbon atoms is there in a 4.0 mg dose of loperamide? (1 Point)
A typical dose of loperamide for an adult is 4.0 mg. What mass of carbon atoms is there in a 4.0 mg dose of loperamide? (1 Point)

Solution
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Answer

0.291 g of carbon atoms. Explanation 1. Determine the molecular formula of loperamide Loperamide's molecular formula is C_{29}H_{33ClN_2O_2}. 2. Calculate the molar mass of loperamide Molar mass = (29 \times 12.01) + (33 \times 1.008) + (1 \times 35.45) + (2 \times 14.01) + (2 \times 16.00) g/mol = 477.04 g/mol. 3. Calculate the number of moles in a 4.0 mg dose Moles = \frac{4.0 \text{ mg}}{477.04 \text{ g/mol}} = \frac{4.0 \times 10^{-3} \text{ g}}{477.04 \text{ g/mol}}. 4. Calculate the mass of carbon atoms Mass of carbon = Moles \times 29 \times 12.01 g/mol.

Explanation

1. Determine the molecular formula of loperamide<br /> Loperamide's molecular formula is $C_{29}H_{33ClN_2O_2}$.<br /><br />2. Calculate the molar mass of loperamide<br /> Molar mass = $(29 \times 12.01) + (33 \times 1.008) + (1 \times 35.45) + (2 \times 14.01) + (2 \times 16.00)$ g/mol = 477.04 g/mol.<br /><br />3. Calculate the number of moles in a 4.0 mg dose<br /> Moles = $\frac{4.0 \text{ mg}}{477.04 \text{ g/mol}} = \frac{4.0 \times 10^{-3} \text{ g}}{477.04 \text{ g/mol}}$.<br /><br />4. Calculate the mass of carbon atoms<br /> Mass of carbon = Moles $\times 29 \times 12.01$ g/mol.
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