1. …Somebody at some point made this. Ehh it’s ok.
Semester 2 Review
…Somebody at some point made this.
Ehh it’s ok.

2. Stoich

4. Stoichiometry Vocab Limiting vs. Excess Reagent
Theoretical vs. Actual Yield
% yield = (Actual yield / Theoretical yield) x 100

5. Thermo.

6. Vocab
Thermochemistry Potential Energy Kinetic Energy Energy Heat Temperature Calorimetry
Enthalpy
Entropy
Hess’s Law
Specific Heat Capacity
Endothermic Reactions
Exothermic Reactions

7. Specific Heat Calculations
q = (m)(c)(ΔT)
heat = mass • specific heat • change in temp
∆𝑇= 𝑇 𝑓𝑖𝑛𝑎𝑙 − 𝑇 𝑖𝑛𝑖𝑡𝑖𝑎𝑙

8. Application of Hess’s Law… Reg.
Find the ΔH for the reaction below, given the following reactions and subsequent ΔH values:
SO3 (g) + H2O (g)  H2SO4 (l)
H2SO4 (l)  H2S (g) + 2 O2 (g) ΔH = kJ
H2O (g)  H2O (l) ΔH = -44 kJ
H2S (g) + 2 O2 (g)  SO3 (g) + H2O (l) ΔH = -207 kJ
Change in Enthalpy = -72.5kJ

9. Application of Hess’s Law… Honors
Calculate the enthalpy of the following chemical reaction: CS2(ℓ) + 3O2(g) ---> CO2(g) + 2SO2(g) Given: C(s) + O2(g) ---> CO2(g) ΔH = kJ/mol S(s) + O2(g) ---> SO2(g) ΔH = kJ/mol C(s) + 2S(s) ---> CS2(ℓ) ΔH = kJ/mol

10. Calculations
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) Enthalpies of formation: CH4: kJ/mol O2: 0.0 kJ/mol CO2: kJ/mol H2O: kJ/mol

11. Calculations
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) Enthalpies of formation: CH4: kJ/mol X 1 mol = kJ O2: 0.0 kJ/mol X 2 mol = 0.0 kJ CO2: kJ/mol X 1 mol = kJ H2O: kJ/mol X 2 mol = kJ

12. Calculations
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g) Enthalpies of formation: ΔH = ( kJ kJ) – ( kJ kJ) ΔH = kJ

13. Molarity

14. Vocab: Be a part of the solution!
Solute: The particles that become dissolved.
Solvent: the dissolving medium (what the solute dissolves in).
Aqueous Solution: solution where the solvent is water.
Concentration: a measure of the amount of solute that is dissolved in a given quantity of solvent.

15. Solution making 101
To reach a specific concentration of solution, we must carefully calculate and measure out both the solute and the solvent.
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑡ℎ𝑒 𝑠𝑜𝑙𝑢𝑡𝑒= 𝑑𝑒𝑠𝑖𝑟𝑒𝑑 𝑚𝑜𝑙𝑎𝑟𝑖𝑡𝑦 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑑𝑒𝑠𝑖𝑟𝑒𝑑 𝑣𝑜𝑙𝑢𝑚𝑒
Volume must be in Liters!

16. Calculations with Dilutions
M1V1 = M2V2
(Molarity)(Volume) = (Molarity)(Volume)

17. Kinetics and Equilibrium

18. Vrooom!
Collision Theory: Particles must collide with proper orientation and enough energy to react.
Factors that affect reactions rates:
Concentration
Surface area
Particle size
Temperature
Catalysts

19. Law of Mass Action
Chemical Equilibrium: a state in which the forward and reverse reactions balance each other because they take place at equal rates.
For the reaction:
𝑗𝐴+𝑘𝐵 ↔𝑙𝐶+𝑚𝐷
Where K is the Equilibrium Constant, and is unitless.
Ignore pure solids and pure liquids with equilibrium.

20. Le Chatelier’s Principle
If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change.
Possible changes:
Concentration
Pressure
Volume
Inert Gas
Temperature

21. Nuclear Chemistry

22. Radiation Radioisotopes: Isotopes with unstable nuclei.
Three types of radiation:
Alpha particles
Beta particles
Gamma rays

23. Nuclear Equations

24. Fission vs. Fusion
Nuclear Fission: the splitting of a nucleus into fragments.
This is accompanied by a very large release of energy.
Nuclear Fusion: the combination of atomic nuclei.
This releases more energy than fission and uses materials that are easier to come by.
The activation energy is around 5,000,000K.

25. Acids and Bases

26. Not so Mathy Bronsted-Lowry acid vs. Bronsted-Lowry base
Conjugate acid and base
Amphoterism
Strong acids
HCl, HBr, HI, HClO4, H2SO4, HNO3
Strong bases
Group I and II hydroxides

27. pH and pOH Calculations

28. Gas Laws

29. Not so Mathy What causes pressure?
What can we use to measure pressure?
Relationships between pressure, volume, temperature and moles of gas.

30. Gas Laws Boyle’s Law PV = PV Charles’s Law V/T = V/T
Gay-Lussac’s Law P/T = P/T
Combined Gas Law PV/T = PV/T
Ideal Gas Law PV = nRT
Dalton’s Law of Partial Pressures Total pressure = Sum of partial
n1/nT = P1/PT