Calcium Chloride and Oxygen

A Guide to Solving Stoichiometry Problems

Truc Tran

What is stoichiometry?

Basically, stoichiometry allows us to convert and find the relationship between the reactant and its product in a chemical equation.

Stoichiometry: What is Stoichiometry?

Balanced Equation

In order to solve stoichiometric problems, you would first need to balance the given chemical equation.


Given the equation Calcium chloride and oxygen.


  1. Decide on the type of reaction that is taking place. For calcium chloride and oxygen, the reaction would be synthesis. There is a rule that states "Reaction of a metal chloride and oxygen produces a metal chlorate." CaCl2 + O2 -> Ca(ClO3)2 or Calcium chloride + Oxygen -> Calcium chlorate should be your current equation.
  2. Next step is to balance the equation. Since both sides already have the same amount of calcium and chlorine, all we need to do is balance the oxygen. Simply add 3 in front of the oxygen on the reactant side to get six of it like in the product. The balanced equation should look like - CaCl2 + 3O2 -> Ca(ClO3)2

Molar mass

Before doing Mole to mole or Mass to mass conversions, it's handy to find the molar mass of the compounds ahead of time. You can get the mass by looking on the periodic table. Just add together the elements and multiply the elements that have a following subscript (Do not include coefficients). For example:


  • Ca = 40.078 g
  • Cl = 35.453 g
  • CaCl2 = 40.078 + 35.453(2) = 110.984 g/mole


  • O2 = 15.999(2) = 31.998 g/mole


  • Ca(ClO3)2 = 40.078 + 2[35.453 + 15.999(3)] = 206.978 g/mole

Mole to Mole Conversions

Formula for mole to mole conversion is:

Mole A (from given)| Mole B (Coefficient)

----------------------------- | Mole A (Coefficient)


Let's say that I got 3.18 moles of CaCl2. This would be my given. So, let's go ahead and plug in the numbers to find O2:


3.18 moles CaCl2|3 moles O2

-------------------------| 1 mole CaCl2


Multiply the top numbers and divide by the bottom to get the mole for O2. The answer will result in 9.54 moles of O2.

Mass to Mass Conversion

Mass to mass is similar to mole to mole, but this time you are looking for the mass. There are more steps to this conversion, though it's pretty simple due to the fact that you only have to plug in the number and solve.


Formula: PT= Periodic table

Mass A (given)|Mole A (always 1)|Mole B (coefficient)|Molar mass B(PT)

---------------------|Molar mass A(PT) |Mole A (coefficient)|Mole B (always 1)


Let's say there's 12.1g of CaCl2:

12.1 g CaCl2| 1 mole CaCl2 | 1 Ca(ClO3)2 | 206.978g Ca(ClO3)2 = 22.6 g of Ca(ClO3)2

------------------|110.984gCaCl2|1 mole CaCl2|1 mole Ca(ClO3)2

Limiting and Excess Reactant

The limiting reactant limits the amount of product that can be made.

Excess reactant is the reactant that you have extra of.

To find the limiting and excess reactant, you have to do mass to mass conversion.

Problems that have 2 givens are usually the ones asking for the limiting and excess reactants.


Let's say there are 12.3g of CaCl2 and 12.3g of O2 :


12.3g CaCl2|1 mole CaCl2|1mole Ca(ClO3)2|206.978g Ca(ClO3)2 = 22.94 g Ca(ClO3)2

----------------|110.984gCaCl2|1 mole CaCl2 | 1 mole Ca(ClO3)2


12.3g O2| 1 mole O2| 1 Ca(ClO3)2| 206.978 g Ca(ClO3)2 = 26.52g Ca(ClO3)2

-------------|31.998g O2|3 mole O2 |1 mole Ca(ClO3)2


CaCl2 is the limiting reactant and O2 is the excess reactant.

Theoretical yield and Percent yield

The calculated/expected yield of product is called the theoretical yield. The theoretical yield is the result of the limiting reactant when solved. CaCl2 was our limiting reactant, so 22.94 g is the theoretical yield.

The amount actually produced is called the actual yield.

To get the percent yield, divide the actual yield by theoretical yield then multiply by 100.


Given the actual yield 25.01 g of Ca(ClO3)2 :

(25.01/22.94) x 100 = 109%


Reasons why the percent yield is not exactly 100%:

  1. Contains impurities if its over 100%
  2. Less than 100% = Product is lost when transferring to a different container.
  3. Wrong measurements