Acetaminophen (C8H9NO2) is the active ingredient in many nonprescription pain relievers. Each tablet contains 500 mg of acetaminophen, and a typical adult dose is two tablets every eight hours.

• Determine the molar mass of acetaminophen (show your work).

• Calculate the number of moles of acetaminophen in a single tablet (show your work).

• Calculate the number of moles of acetaminophen that an adult would have taken if she took three doses of acetaminophen in one day (show your work).

Question

Chemistry

Brady

4 February, 13:58

Acetaminophen (C8H9NO2) is the active ingredient in many nonprescription pain relievers. Each tablet contains 500 mg of acetaminophen, and a typical adult dose is two tablets every eight hours.

• Determine the molar mass of acetaminophen (show your work).

• Calculate the number of moles of acetaminophen in a single tablet (show your work).

• Calculate the number of moles of acetaminophen that an adult would have taken if she took three doses of acetaminophen in one day (show your work).

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Answers (1)

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Ray Stephenson · Answer 1

1) Molar mass C8H9NO2

Element Atomic mass # of atoms mass

g/mol g

C 12 8 12*8 = 96

H 1 9 1*9 = 9

N 14 1 14*1 = 14

O 16 2 16*2 = 32

molar mass = 96 + 9 + 14 + 32 = 151 g/mol

2) Number of mols in a tablet

# of moles = mass / molar mass = 0.500 g / 151 g/mol = 0.003311 moles

3) 3 doses * 2 tablets * 0.003311 moles / tablet = 0.020 moles