Empirical/Molecular, % Comp, the mole

Front

What is an empirical formula?

Back

An empirical formula represents the simplest whole-number ratio of atoms of each element in a compound.

Front

Which of the following is an example of an empirical formula? CH₃COOH, C₆H₁₂O₆, H₂O

Back

H₂O is the empirical formula.

Front

What is a molecular formula?

Back

A molecular formula shows the actual number and kinds of atoms present in one molecule of a compound.

Front

What are the units for molar mass?

Back

The units for molar mass are grams/mole.

Front

How do you calculate the number of moles from mass?

Back

Number of moles = mass (g) / molar mass (g/mol).

Front

How many moles are in 19.82 g of Mg?

Back

0.82 mol Mg.

Front

How many moles are in 16.94 g of water (H₂O)?

Back

0.9401 mol H₂O.

Front

What is the molar mass of water (H₂O)?

Back

The molar mass of water is approximately 18.02 g/mol.

Front

What is the difference between empirical and molecular formulas?

Back

Empirical formulas show the simplest ratio of elements, while molecular formulas show the actual number of atoms.

Front

If a compound has a molecular formula of C₆H₁₂O₆, what is its empirical formula?

Back

The empirical formula is CH₂O.