1. Warm Up #6 Balance the following:
__H3PO4(aq) + __NaOH(aq)  __HOH(ℓ) + __Na3PO4(aq)
Write the noble gas notation Silver (Ag), and also write the orbital notation (the arrows) for it.
You are given 89.6 grams of Fe2O3. How much of this amount is purely Iron (Fe)?

2. Chapter 12.1 Stoichiometry

3. Stoichiometry…big word, review topic
Why we balance?
Law of Conservation of Mass (mass/matter can not be created/destroyed)
Stoichiometry – using balanced equations to find out how much product is formed from reactants
How? MOLE-to-MOLE RATIOS

4. Ex. 3H2(g) + N2(g)  2NH3(g)
Mole to Mole Ratio – the amount of moles of one thing compared to the other.
__ to __ ratio
USE COEFFICIENTS
H2 to NH3 ratio = 3 to 2 ratio
H2 to N2 ratio = 3 to 1 ratio

5. Ex. 3H2(g) + N2(g)  2NH3(g) (at STP) what this equation tells us
Ratio: 3 mol H2 to 1 mol N2 to 2 mol NH3
Mass: 3(2.02 g) + (28.02 g) = 2 (17.04 g)
34.08 g = g
Volume: 3 mol H2 = (3 x 22.4L) = 67.2 L H2 H2 N2
NH3

6. Converting: Grams H2 into mol NH3 3H2(g) + N2(g)  2NH3(g)
You are given: 34 grams H2. How many mol NH3 are made? USE T-CHARTS.
Start with 34 grams H2
Convert into mol (ALWAYS). (1 mol H2 = 2.02 g)
Periodic table
Mole to Mole Ratio (3 mol H2 = 2 mol NH3)
Balanced equation
DONE

7. Grams A to Grams B Flow Chart
Moles A
Moles B

8. Grams A to Grams B T-Chart
Moles A
Moles B
Grams B
Grams A
Grams A
Moles B
Moles A
Mole to Mole Ratio
Given
Periodic Table
Periodic Table