1. __C3H8(g) + __O2(g) ⇌ __CO2(g) + __H2O(g)
Warm Up #7
If the Ksp for Iron (II) Phosphate is 8.4x Calculate the molar solubility for this substance.
Calculate the heat of formation for the following reaction:
__C3H8(g) + __O2(g) ⇌ __CO2(g) + __H2O(g)
If the reaction begins at kJ and has an activation energy of 200 kJ. Draw the above reaction in an energy pathway.

2. __C3H8(g) + __O2(g) ⇌ __CO2(g) + __H2O(g)
Warm Up #6
Calculate the heat of formation for the following reaction:
__C3H8(g) + __O2(g) ⇌ __CO2(g) + __H2O(g)
If the reaction begins at kJ and has an activation energy of 200 kJ. Draw the above reaction in an energy pathway.
Write a k equation for the reaction above. If the concentration of the reactants is 0.59M and the products are 0.23M, what does k equal? Are the reactants or products favored?

3. Chapter 18.4 Hess’s Law

4. How Hess’s Law Works You will be given: Final reaction
A number of sub-steps (ΔH given for each step)
Your job: eliminate all of the unnecessary compounds to get final reaction.
You can: reverse reaction (given ΔH changes signs)
AND/OR
multiply by a coefficient (given ΔH multiplies by that amt)
Anything the SAME on left and right side can CROSS CANCEL.

5. Original Steps: 1) C(s) + O2(g)  CO2(g) ` ΔH = -393.5kJ
FINAL: 2 CO (g) + O2 (g)  2 CO2(g)
Steps:
1) C(s) + O2(g)  CO2(g) ` ΔH = kJ
2) 2 C(s) + O2(g)  2 CO(g) ΔH = kJ

6. Changes Steps: 1) C(s) + O2(g)  CO2(g) ` ΔH = -393.5kJ
FINAL: 2 CO (g) + O2 (g)  2 CO2(g)
Steps:
1) C(s) + O2(g)  CO2(g) ` ΔH = kJ
DOUBLE THE REACTION
2) 2 C(s) + O2(g)  2 CO(g) ΔH = kJ
SWITCH THE DIRECTION

7. Revised Steps: 1) C(s) + O2(g)  CO2(g) ` ΔH = -393.5kJ
FINAL: 2 CO (g) + O2 (g)  2 CO2(g)
Steps:
1) C(s) + O2(g)  CO2(g) ` ΔH = kJ
2 C(s) + 2 O2(g)  2 CO2(g) ΔH = kJ
2) 2 C(s) + O2(g)  2 CO(g) ΔH = kJ
2 CO(g)  2 C(s) + O2(g) ΔH = 221.0kJ
ΔH = (-787.0) + (221.0) = kJ 1

8. COPY!