Culminating assesment for semester: Reaction in a Bag
Group lab report due on Thursday, May 13
Parts 6-12 of Review Assignment (See below.) due Friday, May 14
Remainder of Review Assignment due on Monday, May 17
Final Exam Review:
1. Define: Boyle's Law, Charles Law, Gay-Lussac's Law, The combined gas law, Dalton's Law of Partial Pressure, Avogadro's Principle, Ideal Gas Law, LeChatelier's principle,
2. Explain significance of these numbers: 0 K, 0 oC, 100 oC, 22.4, 101.3, 273, 760
3. Define: alkene, alkyne, Avogadro’s number, catalyst, density, diffusion, effusion, empirical formula, endothermic, entropy, equilibrium, equilibrium vapor pressure, exothermic, heat, oxidation-reduction reaction, molarity, molecular formula, pressure, saturated hydrocarbon, unsaturated hydrocarbon, saturated solution, unsaturated solution, supersaturated solution, soluble, solubility, solute, solution, solvent, suspension, STP, temperature, Arrhenius acid & base (& characteristics), Bronsted acid & base, Lewis acid & base, monoprotic acid, diprotic acid, triprotic acid, polyprotic acid, amphoteric.
4. Copy Figure 17-3 on page 597 and Figure 14.2 on page 492. Make sure you understand them.
5. Write and label the equation for the self ionization of water.
6. Composition Stoichiometry:
A. What is each element's percent composition in MgCO3?
B. A hydrocarbon is 82.6 % carbon and 17.4% H. What is the empirical formula of the compound?
C. The molar mass of the compound in “B” is 58 g/mol. What is the molecular formula of the compound?
7. Reaction Stoichiometry Problems:
2 NaCl + Pb(NO3)2 à 2 NaNO3 + PbCl2
A. How many grams of sodium chloride are needed to react with 0.234 moles of lead(II) nitrate?
B. How many grams of lead(II) chloride are produce from 27.33 grams of lead(II) nitrate?
C. If the experimental/actual yield is 21.45 g, calculate the percent yield.
8. Molarity problems:
A. Find the molarity of a 2.4 L solution made with 20.5 g of sulfuric acid?
B. How many grams of magnesium hydroxide are required to make 1.23 L of 0.45 M solution.
9. pH problems:
A. If the pH = 4.6, calculate the pOH, [H+], [OH-]. Is the solution acidic, basic or neutral? What color is the solution if the indicator phenolphthalein is added?
B. If the [OH-] = 7 x 10-10 M, calculate pH, pOH, [H+]. Is the solution acidic, basic or neutral? What effect will the solution have on both colors of litmus paper?
10. Predict the products and balance the reaction. Label the acid, the base, the salt. Identify the conjugate pairs.
HNO3 + Mg(OH)2 à
11. Gas Law problems:
A. What is the volume of 21.6 g of nitrogen at STP?
B. A sample of gas has a volume of 15.7 mL at 1.25 atm and 25oC. What is the new volume at 50. oC and 1.00 atm?
C. What is the mass of 2.5 L of ammonia gas at 22 oC and 56 kPa?
12. Putting it all together: If 20.0 g of potassium bicarbonate reacts with 95.0 mL of 2.50 M acetic acid, what volume of gas is released at 790 mm Hg and 65 oC? (Hint: Write a balanced reaction and then find the limiting reactant.)
13. What factors affect the rate of a reaction?
14. Define equilibrium, kinetic molecular theory, collision theory, activation energy, catalyst.
15. How much energy is required to completely melt 26.0 grams of ice? (ΔH = molHf) Hf for water = 6.00 kJ/mol
16. How much energy is required to raise the temperature of 25.0 g of water from 23oC to 97oC?
17. Write the equilibrium expression for the formation of ammonia from nitrogen and hydrogen. (Hint: write the balanced chemical equation first.)
18. If the concentration of nitrogen is 0.134M, the concentration of hydrogen is 0.264M, and the concentration of ammonia is 0.273M, what is the equilibrium constant?
19. In the reaction C2H4O (g) + heat ß à CH4 (g) + CO (g)
a) What effect will increasing the temperature have on the equilibrium?
b) What effect will adding CH4 have?
c) What effect will increasing the pressure have?
d) What effect will removing CO have?
20. Organic nomenclature
