1. Semester 2 Review

2. THE MOLE
Using the mole and molar mass, make conversions between moles, mass and number of particles.
Use molar mass to calculate percent composition, empirical formula, and molecular formula.

3. How many moles are equivalent to 2.58x1024 atoms of gold?
Answer: mol

4. What is the molar mass of ammonium phosphate? (NH4)2SO4
Answer: g/mol

5. A chemical used in batteries is 63. 0% Manganese and 37. 0% Oxygen
A chemical used in batteries is 63.0% Manganese and 37.0% Oxygen. What is the empirical formula?
Answer: MnO2

6. The empirical formula of a compound is P2O5
The empirical formula of a compound is P2O5. The molar mass of the compound is 284 g/mol. What is the molecular formula?
Answer: P4H10

7. Calculate the percent composition of copper (I) sulfide (Cu2S).
Answer: % Cu and 20.15% S

8. STOICHIOMETRY Convert from one substance to another
Determine amount of reactant/product
Determine limiting reactant/excess
Determine theoretical & percent yield
Use density to convert between substances

9. Using the following balanced chemical reaction:
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)
How many molecules of oxygen are needed to react with 2.45 mol of CH4?
2.95 x 1024 molecules O2

10. What volume of hydrogen gas is produced if there are 112 g NH3 in the following reaction at 1.15 atm and 23 degrees Celsius? 2NH3(g)  N2(g) + 3H2(g)
208 L

11. If reactant “A” runs out before reactant “B” and the reaction stops, then reactant “A” is known as the …
LIMITING REACTANT

12. Using the following reaction, 2Na(s) + 2H2O(g)  2NaOH(aq) + H2(g) If you have 15.2 g of Na and 12.5 g of H2O, how many grams of H2 gas can be made?
0.658 g H2

13. If the theoretical yield of a reaction is 125 g and the actual yield is 115 g, what is the percent yield?
92.0 %

14. GASES
STP values
Use gas laws to determine pressure, volume, and temperature.
Use gas laws to determine moles or grams or molar mass.
Use gas laws and stoich. to determine amounts of reactants and products.

15. What are STANDARD conditions for gases?
0oC or 273 K and 1 atm or kPa pressure

16. A sample of gas has a volume of 25 mL and a temperature of 65oC
A sample of gas has a volume of 25 mL and a temperature of 65oC. What will the volume be if the temperature is raised to 125oC?
29 mL

17. How many grams of gas are present in a sample that has a molar mass of 70.0 g/mol and occupies 2.00 L at 117 kPa and 35.1oC?
6.36 g

18. What is the pressure in atmospheres of a 0
What is the pressure in atmospheres of a mol sample of helium gas at a temperature of 20.0oC if its volume is L?
5.14 atm

19. Calculate the mass of solid ammonium nitrate that must be used to obtain L of dinitrogen monoxide gas at STP.
NH4NO3(s)  N2O(g) + 2H2O(g)
0.357 g

20. SOLUTIONS Solubility (“like dissolves like”) Concentration (molarity)
Vocab
unsaturated, saturated, supersaturated, soluble, insoluble, miscible, immiscible
Electrolytes and Non-Electrolytes

21. What is the molarity of a 500
What is the molarity of a 500. mL solution that contains 125 g of sodium hydroxide?
6.25 M

22. How many milliliters of a 0
How many milliliters of a M solution of sodium thiosulfate, Na2S2O3, contain mol of Na2S2O3?
0.412 L

23. Identify which of the following substances are soluble in water: CaF2 Al C3H8 CCl4

24. For which type of substance does an increase in pressure increase solubility?
gases

25. saturated, unsaturated, supersaturated
A ____________ solution contains the maximum amount of solute it can hold. An __________ solution contains less than the maximum amount. A ____________ solution contains more than the maximum amount.
saturated, unsaturated, supersaturated

26. RATES Collision Theory Factors that Affect Rate
How and Why Rate Changes Over Time
Catalysts

27. Describe collision theory.
Reactants must collide (with enough energy and the correct orientation) in order to produce an activated complex and form product.

28. How does a catalyst increase the rate of a reaction?
It lowers the activation energy by creating an alternate path.

29. How does the rate of a reaction change over time?
The rate slows down because the concentration of the reactants decreases over time.

30. EQUILIBRIUM Completion vs. Reversible
Rates of Reactions at Equilibrium
Keq
LeChatelier’s Principle
Equilibrium Expressions
Calculating K
Ksp

31. A ________ reaction is represented by , while a ______ reaction is represented by  .
completion, reversible

32. 2 NO2 (g)  N2O4 (g) + Energy What happens if we…
Lower the Temperature
Increase N2O4
Decrease NO2
Increase Pressure
Increase Volume
Shift right
Shift left

33. What does it mean if the reaction shifts to the right
What does it mean if the reaction shifts to the right? How would the amounts of reactants and products change?
The reactions favors the forward reaction so the amounts of reactants decrease and products increase.

34. Equilibrium Expressions
Write the equilibrium constant for the following reaction:
N2 (g) + 3 H2(g)  2 NH3(g)
Keq = [NH3]2
[N2][H2]3

35. Calculate Keq for the reaction below if [S2] = 0. 0540 M, [H2] = 0
Calculate Keq for the reaction below if [S2] = M, [H2] = M, and [H2S] = M. 2 H2S (g)   2 H2(g) + S2(g)
Keq = 2.27 x 10-3

36. What does a large value for Keq mean? A small value for Keq?
Large means products are favored at equilibrium while small means reactants are favored

37. Which of the substances below is most soluble. Least soluble. CaF2 – 3
Which of the substances below is most soluble? Least soluble? CaF2 – 3.5 x PbCrO4 – 2.3 x Al(OH)3 – 4.6 x MgCO3 – 6.8 x 10-6
Most soluble = MgCO3
Least soluble = Al(OH)3

38. ACIDS & BASES Electrolytes and Strong vs. Weak Bronsted – Lowry
Amphoprotic – Amphoteric
pH calculations
Titrations

39. What is the pH of 0.00025M HCl (a strong acid)?
Answer: 3.60

40. What is the concentration of H+ if the pOH is 7.82?
6.61 x 10-7M

41. What word is used to describe substances that can act as an acid or a base?
Answer: Amphoteric

42. Strong acids and bases ionize ___________ while weak acids and bases ionize __________.
completely, partially

43. HSO4- (aq) + H2O (l)  H3O+ (aq) + SO42- A B CA CB
Label the A, B, CA, CB in the following reaction: HSO4- (aq) + H2O (l)  H3O+ (aq) + SO42-
HSO4- (aq) + H2O (l)  H3O+ (aq) + SO42-
A B CA CB

44. A student titrates 40.0 mL of an H2SO4 solution of unknown concentration with mL of a M NaOH solution. What is the molarity of the H2SO4 solution?
H2SO4 + 2 NaOH  2 H2O + Na2SO4
[HCl] = M