Answer:
[tex]9.696\cdot10^{-4} mol[/tex]
Explanation:
Let's firstly define how we calculate the number of moles. Moles are defined as the ratio between the mass of a substance (in this case, mass is 200.0 mg, or 0.2000 g) and the molar mass of that substance (this is what we'll need to determine).
Given the molecular formula of ibuprofen, let's calculate its molar mass adding the molar masses of each element and multiplying by the subscripts given in the molecular formula:
[tex]M_{C_{13}H_{18}O_2}=13M_C+18M_H+2M_O=13\cdot 12.011 \frac{g}{mol}+18\cdot1.00784\frac{g}{mol}+2\cdot16.00\frac{g}{mol}= 206.28\frac{g}{mol}[/tex]
Now the solution is straightforward, dividing the mass in grams:
[tex]200.0 mg\cdot\frac{1 g}{1000 mg}=0.2000 g[/tex]
by the molar mass will yield moles:
[tex]n=\frac{m}{M}=\frac{0.2000 g}{206.28\frac{g}{mol}}=9.696\cdot10^{-4} mol[/tex]
The number of mole of ibuprofen in a single tablet is 9.695×10¯⁴ mole
The mole of a substance is related to it's mass and molar mass according to the following equation
Mole = mass /molar mass
With the above formula, we can obtain the mole of ibuprofen in a single tablet
•Mass of 1 tablet = 200 mg = 200×10¯³ g
•Molar mass of Ibuprofen = 206.29 g/mol
•Mole of 1 tablet =?
Mole = mass /molar mass
Mole of 1 tablet = 200×10¯³ / 206.29
Mole of 1 tablet = 9.695×10¯⁴ mole
Therefore, the mole of 1 tablet of ibuprofen is 9.695×10¯⁴ mole
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