How many moles of c9h8o4 are in a 0.600 g tablet of aspirin?

[tex]\boxed{{\text{0}}{\text{.0033}}\;{\text{mol}}}[/tex] of [tex]{{\text{C}}_{\text{9}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{4}}}[/tex] are present in 0.600 g tablet of aspirin.

Further Explanation:

Mole is a measure of the amount of substance. It is defined as the mass of a substance that has the same number of fundamental units as there are atoms in 12 g of carbon-12. Such fundamental units can be atoms, molecules or formula units.

In step 1, we have to calculate the molar mass of aspirin. Molar mass of aspirin can be calculated by using the equation 1.

Step 1: The molecular formula of aspirin is [tex]{{\text{C}}_{\text{9}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{4}}}[/tex]. Its molar mass is calculated as follows:

[tex]{\text{Molar mass of }}{{\text{C}}_{\text{9}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{4}}}=\left[\begin{gathered}{\text{9}}\left( {{\text{Atomic mass of C}}}\right)+\hfill\\{\text{8}}\left( {{\text{Atomic mass of H}}}\right)+\hfill\\{\text{4}}\left( {{\text{Atomic mass of O}}}\right)\hfill\\\end{gathered}\right][/tex] …… (1)

The atomic mass of C is 12 g.

The atomic mass of H is 1 g.

The atomic mass of O is 16 g.

Substitute these values in equation (1).

[tex]\begin{aligned}{\text{Molar mass of }}{{\text{C}}_{\text{9}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{4}}}&=\left[{9\left( {{\text{12}}} \right)+8\left({\text{1}}\right)+4\left({{\text{16}}}\right)} \right]\\&=108+8+64\\&= {\mathbf{180}}\;{\mathbf{g/mol}}\\\end{aligned}[/tex]

In step 2, the molar mass calculated in step 1 is used to calculate the number of moles of aspirin. The number of moles of aspirin is calculated by using equation (2).

Step 2: The formula to calculate the moles of aspirin [tex]\left( {{{\mathbf{C}}_{\mathbf{9}}}{{\mathbf{H}}_{\mathbf{8}}}{{\mathbf{O}}_{\mathbf{4}}}}\right)[/tex] is as follows:

[tex]{\text{Moles of }}{{\text{C}}_{\text{9}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{4}}}=\dfrac{{{\text{Given mass of }}{{\text{C}}_{\text{9}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{4}}}}}{{{\text{Molar mass of }}{{\text{C}}_{\text{9}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{4}}}}}[/tex] ...... (2)

The given mass of aspirin is 0.600 g.

The molar mass of aspirin is 180 g/mol.

Substitute these values in equation (2)

[tex]\begin{aligned}{\text{Moles of }}{{\text{C}}_{\text{9}}}{{\text{H}}_{\text{8}}}{{\text{O}}_{\text{4}}}&=\left({0.600\;{\text{g}}} \right)\left( {\frac{{1\;{\text{mol}}}}{{180\;{\text{g}}}}}\right)\\&={\text{0}}{\text{.003333}}\\&\approx {\mathbf{0}}{\mathbf{.0033}}\;{\mathbf{mol}}\\\end{aligned}[/tex]

Learn more:

1. Calculate the moles of chlorine: https://brainly.com/question/3064603

2. What is the number of moles of ions in HCl solution? https://brainly.com/question/5950133

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Mole concept

Keywords: moles, aspirin, 0.600 g, C9H8O4, molar mass, carbon-12, amount of substance, mass of substance, formula units, 180 g/mol, 0.0033 mol.