# Stoichiometry

# Molecular Mass

Now that we know all about atomic masses we can move on to bigger and better things…molecules. (Maybe not

What's the molecular mass of water (H

molecular mass H

Where do we find the atomic mass of H and O? Whip out your favorite periodic table. We know, we heart the periodic table, too.

molecular mass H

From the molecular mass we can determine the

We just calculated the molecular mass of water to be 18.02 amu. Lucky for us (thanks again to the chemistry gnomes), its molar mass is 18.02 g. That means 1 mole of water is equal to 18.02 g.

Let's put this stuff into perspective. Roughly 1.2 tablespoons of water is equal to 18.02 grams. Those 18.02 grams represent one mole of water. That means every 1.2 tablespoons of water contains 6.023 x 10¬

Methane = CH

First of all, we are given grams of CH

Molar mass of CH

Note: we multiply by 4 because there are 4 hydrogen atoms in each CH

Molar mass of CH

Molar mass of CH

Therefore our conversion factor is:

What gives? Why do we need two conversion factors? We don't. We just need to use the conversion factor that will give us the right units in the end. Remember, if a unit appears above

To solve we now write:

We're officially masters of molecular masses.

*better*. We don't want to offend all the atoms out there.) If we know the atomic masses of individual atoms, we can easily calculate the mass of a molecule. The**molecular mass**(sometimes called the**molecular weight**) is just the sum of the atomic masses in a molecule.What's the molecular mass of water (H

_{2}O)? To calculate the molecular mass we add together the atomic mass of two hydrogen atoms and one oxygen atom:molecular mass H

_{2}O = 2(atomic mass of H) + atomic mass of OWhere do we find the atomic mass of H and O? Whip out your favorite periodic table. We know, we heart the periodic table, too.

molecular mass H

_{2}O = 2(1.008 amu) + 16.00 amu = 18.02 amuFrom the molecular mass we can determine the

**molar mass**of a molecule. Just as the name suggests the molar mass is the mass (in grams) of one mole of a compound. We don't even need a calculator to compute between molecular mass and molar mass…the values are numerically the same. The molar mass of a compound (in grams) is numerically equal to its molecular mass (in amu).We just calculated the molecular mass of water to be 18.02 amu. Lucky for us (thanks again to the chemistry gnomes), its molar mass is 18.02 g. That means 1 mole of water is equal to 18.02 g.

Let's put this stuff into perspective. Roughly 1.2 tablespoons of water is equal to 18.02 grams. Those 18.02 grams represent one mole of water. That means every 1.2 tablespoons of water contains 6.023 x 10¬

^{23}H_{2}O molecules. Think about that next time you down a glass of water. Who knew we were drinking so many molecules?### Sample Problem

One of the main components of natural gas is methane (CH_{4}). How many moles of CH_{4}are present in 4.83 g of CH_{4?}Methane = CH

_{4}First of all, we are given grams of CH

_{4}and asked to solve for moles of CH_{4}. This means we need a conversion factor between grams and moles. Once again, the periodic table is your BFF. We need to collect the atomic masses of carbon and hydrogen from the periodic table and then calculate the molecular mass of CH_{4 }by simple addition.Molar mass of CH

_{4}= atomic mass carbon + 4(atomic mass of hydrogen)Note: we multiply by 4 because there are 4 hydrogen atoms in each CH

_{4}.Molar mass of CH

_{4}= 12.01 g + 4(1.008 g)Molar mass of CH

_{4}= 16.04 gTherefore our conversion factor is:

What gives? Why do we need two conversion factors? We don't. We just need to use the conversion factor that will give us the right units in the end. Remember, if a unit appears above

*and*below the fraction line they will cancel each other out. We need to arrange the conversion factor in whichever way will allow us to do that.To solve we now write:

We're officially masters of molecular masses.

### Brain Snack

Jeremias Benjamin Richter (1762-1807) (not to be confused with Andy Richter) was the first guy to lay down the principles of stoichiometry.^{4}He thought that chemistry could be seen as just another version of applied math. In his own words, "Stoichiometry is the science of measuring the quantitative proportions or mass ratios in which chemical elements stand to one another." You can read more about this brainy dude here.