From the given molar mass and empirical formula of several compounds, find the molecular formula of each compound. b. CCl, 284.77 g/mol

Verified step by step guidance

1. Determine the molar mass of the empirical formula CCl.
2. Calculate the molar mass of CCl by adding the atomic masses of carbon (C) and chlorine (Cl).
3. Divide the given molar mass of the compound (284.77 g/mol) by the molar mass of the empirical formula (CCl) to find the ratio.
4. Multiply the subscripts in the empirical formula by the ratio obtained in the previous step to find the molecular formula.
5. Write the molecular formula using the new subscripts obtained from the multiplication.

Key Concepts

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a molecule based on its chemical formula. Understanding molar mass is crucial for converting between grams and moles, which is essential for determining the molecular formula from the empirical formula and given mass.

Empirical Formula

The empirical formula represents the simplest whole-number ratio of the elements in a compound. It provides essential information about the composition of the compound but does not indicate the actual number of atoms in a molecule. To find the molecular formula, one must first determine the empirical formula and then use the molar mass to scale it up to the actual molecular composition.

Molecular Formula

The molecular formula indicates the actual number of each type of atom in a molecule of a compound. It can be derived from the empirical formula by multiplying the subscripts by a whole number, which is determined by dividing the compound's molar mass by the molar mass of the empirical formula. This concept is vital for understanding the true structure and properties of the compound.