Ibuprofen, an anti-inflammatory drug in Advil, has the formula C₁₃H₁₈O₂ (7.1, 7.2, 7.3) d. How many moles of ibuprofen contain 1.22 x 10²³ atoms of C?

Verified step by step guidance

1. Step 1: Identify the number of carbon atoms in one molecule of ibuprofen.
2. Step 2: Use Avogadro's number (6.022 x 10^{23} atoms/mol) to determine the number of moles of carbon atoms in 1.22 x 10^{23} atoms of C.
3. Step 3: Calculate the number of moles of ibuprofen by dividing the moles of carbon atoms by the number of carbon atoms per molecule of ibuprofen.
4. Step 4: Set up the equation: (moles of C atoms) / (13 C atoms/molecule) = moles of ibuprofen.
5. Step 5: Solve the equation to find the moles of ibuprofen.

Key Concepts

Moles and Avogadro's Number

A mole is a unit in chemistry that represents 6.022 x 10²³ entities, such as atoms or molecules. This number, known as Avogadro's number, allows chemists to convert between the mass of a substance and the number of particles it contains. Understanding this concept is crucial for solving problems involving quantities of substances in chemical reactions.

Molecular Formula

The molecular formula of a compound indicates the number and type of atoms present in a molecule. For ibuprofen, C₁₃H₁₈O₂ shows that each molecule contains 13 carbon (C) atoms, 18 hydrogen (H) atoms, and 2 oxygen (O) atoms. This information is essential for determining the number of moles based on the number of atoms.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows for the calculation of how much of one substance is needed or produced based on the amounts of others. In this context, stoichiometry helps in converting the number of carbon atoms into moles of ibuprofen.