1. Stoichiometry Calculating Masses of Reactants and Products

2. Stoichiometry Stoichiometry refers to the relative quantities of moles and calculations that make use of mole ratios. Consider: Ammonia reacts with oxygen to form water and nitrogen monoxide.

3. Stoichiometry Strategy 4NH 3 + 5O 2 → 6H 2 O + 4NO

4. 4NH 3 + 5O 2 → 6H 2 O + 4NO Mole to Mole Stoichiometry How many moles of H 2 O are produced if 0.176 mol of O 2 are used? How many moles of NO are produced in the reaction if 17 mol of H 2 O are also produced?

5. 4NH 3 + 5O 2 → 6H 2 O + 4NO Mole to Mass Stoichiometry How many grams of H 2 O are produced if 1.9 mol of NH 3 are combined with excess oxygen? How many grams of O 2 are required to produce 0.3 mol of H 2 O?

6. 4NH 3 + 5O 2 → 6H 2 O + 4NO Gravimetric Stoichiometry (Mass to Mass) How many grams of NO is produced if 12g of O 2 is used? Assume O 2 is the limiting reagent.

7. Gravimetric Stoichiometry Strategy Write a BALANCED chemical equation Write the known masses directly underneath each compound. Determine the Molar Mass of all substances involved. Calculate the number of moles of the substance of known mass. Use the mole ratio in your balanced chemical equation to determine the amount in moles of your desired substance Convert the amount in moles to mass

8. Demo Water initiates a reaction between 2.4 grams of silver nitrate powder and calcium powder, resulting in a bright flash, heat and smoke. Predict the following: – Mass of calcium powder required – Mass of products