1. Stoichiometry Objectives:
1. Define stiochiometry and describe its significance.
2. Explain the relationship between stoichiometry and balanced chemical equations.

2. Stoichiometry
Stoichiometry is simply the use of molar ratios to calculate the reactants and products in a balanced equation.
Used to predict the quantity and mass of products from known reactants in any equation using stiochiometric relationships.
Predictions can be based on moles, mass, particles, or volume. The trick to is to use the ratio of moles to solve all the different types of problems.
Follows the Laws of Conservation of mass, matter, & energy

3. Interpreting balanced equations:
Mole - Mole Conversions
CH4 + 2O2 g CO2 + 2H2O
Consider the balanced equation above.
Reactants:
1 mole of CH4 - contains 1 mole Carbon and 4 moles Hydrogen
reacts with 2 moles of O2 - contains 4 moles Oxygen
Products:
1 mole CO2 - contains 1 mole Carbon and 2 moles Oxygen
2 moles of H2O - contains 4 moles Hydrogen and 2 mole Oxygen
Stoichiometry is just like reading a recipe and should be approached the same way. The above recipe calls for 1 part methane to be mixed with 2 parts oxygen to produce 1 part carbon dioxide and 2 parts water.

4. Solving Mole to Mole conversions
The Mole to Mole conversion is the central step in All stoichiometry calculations
Given moles multiplied by molar ratio of substances

5. Practice
How moles of methane would you mix with 10 moles O? (remember that the mole ratio is 2:1)
A. 2.5 B. 5 C. 10 D. 20 (answer is at the bottom)
Math solution: 10mol O x (1mol CH4 / 4mol O) = ?
How many moles of CO2 would this produce?
Math solution: 10mol O x (1mol CO2 / 4mol O) = ?
How many moles of H2O would this produce?
Math solution: 10mol O x (2mol H2O / 4mol O) = ?
How would the problem be different if you started with 10 moles O2?
answers: A, A, B