Using the models of the molecules (black = C, white = H, yellow = S, green = Cl), determine each of the following for models of compounds 1 and 2: (7.1, 7.2, 7.3)1.
2.
c. number of moles in 10.0 g

Verified step by step guidance

1. Identify the elements in each molecule using the color code: black = C, white = H, yellow = S, green = Cl.
2. For the first molecule (top), identify the elements: it consists of two yellow atoms and one red atom, indicating it is likely sulfur dioxide (SO2).
3. For the second molecule (bottom), identify the elements: it consists of four black atoms and six white atoms, indicating it is likely cyclobutane (C4H6).
4. Calculate the molar mass of each compound: for SO2, add the atomic masses of sulfur and two oxygens; for C4H6, add the atomic masses of four carbons and six hydrogens.
5. Use the formula: number of moles = mass (g) / molar mass (g/mol) to find the number of moles in 10.0 g of each compound.

Key Concepts

Molecular Composition

Molecular composition refers to the types and numbers of atoms that make up a molecule. In the context of the question, understanding the molecular formulas of the compounds represented by the models is essential. For example, the top model likely represents a compound containing sulfur (S) and chlorine (Cl), while the bottom model represents a carbon (C) compound, possibly a hydrocarbon. Identifying these components is crucial for further calculations.

Moles and Molar Mass

A mole is a unit in chemistry that represents 6.022 x 10²³ entities, such as atoms or molecules. Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To determine the number of moles in a given mass of a compound, the formula used is: moles = mass (g) / molar mass (g/mol). This concept is vital for solving the question regarding the number of moles in 10.0 g of the compounds.

Stoichiometry

Stoichiometry is the area of chemistry that deals with the relationships between the quantities of reactants and products in chemical reactions. It allows chemists to predict how much of each substance is needed or produced in a reaction. In this question, stoichiometry will be important for understanding how to relate the number of moles calculated from the mass of the compounds to their molecular formulas and potential reactions.