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.
Balanced Equation
Given the equation Calcium chloride and oxygen.
- 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.
- 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
- 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
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
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
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 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%:
- Contains impurities if its over 100%
- Less than 100% = Product is lost when transferring to a different container.
- Wrong measurements