Potassium Chloride + Oxygen

Assigned Reaction : KCl + O2

Balanced Equation: 2KCl(s) + 3O2(g) ------> 2KClO3(aq)

Type of reaction : Synthesis

Molar Mass of each Reactant and Product:

KCl : 74.45 g/mol

O2: 31.98 g/mol

KClO3: 122.42 g/mol

What is Stoichiometry ?

Stoichiometry is a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data.
Stoichiometry: Chemistry for Massive Creatures - Crash Course Chemistry #6

Mole to Mole Conversion

1.17 KCl will be Mass A.

Then the coefficient of KCl (2) over the coefficient of KClO3 (2)

Then Multiply across the top and Divide by the bottom,

You should end up with 1.17 Mole KClO3

Mass to Mass Conversions

12.1 g KCl (Mass A)

74.45 KCl (Molar Mass of KCl) Over 1 Mole KCl

Coefficient of KClO3 Over the Coefficient of KCl

2 KClO3 over 2 KCl

1 Mole KClO3 over 122.42 g/mol KCl

Then Multiply across the top and then Divide by the Bottom.

You should end up with 19.89 g of KClO3

Limiting and Excess Reactant

The Limiting and Excess equation is to find the Theoretical Yield. You will also find out which is your limiting reactant, the reactant that you will run out of first and then you're excess reactant the reactant that you will have left over.

Using 12,3 as our mass of bother reactants you just do a Mass to Mass Conversion of both of your reactants to find the mass of Product.

Theoretical Yield

My Theoretical Yield Was 20.23g KClO3

My Excess Reactant was 12.3 g O2

My Limiting Reactant was 12.3g KCl

Percent Yield

Actual Yield: 19.85g KClO3

Actual Yield Over Theoretical Yield

Multiply by 100

Percent Yield: 98%