# Stoichiometry Tutorial

## A REACTION? WHOA!

CaO+Co₂ (Calcium Oxide + Carbon Dioxide) make CaCo₃ (Calcium Carbonate)

## WHAT TYPE OF REACTION IS THIS?

This is a synthesis reaction because two elements or compounds are joined together to create a compound. Cao+Co₂ ---> CaCo₃ (Calcium Carbonate + Carbon Dioxide ----> Calcium Carbonate)

## How to Balance an equation

To balance an equation, you have to have the same amount of each element on both side.

(s) is for solid, (l) is for liquid, and (g) is for gas.

CaO (s) + CO₂ (g) ----> CaCo₃ (s)

## IUPAC Naming

CaO= Calcium Oxide

CO2= Carbon Dioxide

## Molar Mass

CaO= 56.0774 g/mol

CO₂= 44.01 g/mol

To find the molar mass, you take the atomic weight and multiply it by how many it has.

## Converting mole to mole

To convert moles to moles you need to know the ratio of two products or reactants in their chemical reaction.

Example. If you have 11.30 Moles of CaO and you're trying to figure out how many moles of CaCo₃ you have.

Take the given (11.3 mols) than multiply it by the mol ratio, in this case that means you have 11.30 moles of CaCo₃

## Mass to Mass

To get from mass to mass (from reactant xyz to reactant abc)

Follow the steps from mole to mole conversions, however, you must divide your second substance by your first substance with a value of 1.

For example,

4.13 grams of Co₂ will convert to 9.39 grams of CaCo₃

After the mole conversion, you would do 100.086 grams CaCo₃ over 1 mole of Co₂

## Limiting and Excess Reactant

The limiting reactant limits the numerical amount of the final product. Excess reactant is the amount that the product is produced.

## Theoretical Yield

Theoretical yield is how much you can make with the two reactants, to find the theoretical yield you multiply the moles of the limiting reactant by the ratio of it and the final product.

## Percent Yield

The percentage yield is the percent your product is made from. So mass of actual yield / mass of the theoretical yield x 100 (percent)