FINAL EXAM in Chemistry will cover the majority of the content covered throughout the year. You may use (1)3 “X 5” note card which you will have 5 minutes to prepare before beginning the exam. You may not pre-prepare your note card.
Given: Periodic table, Solubility chart, Common Polyatomic Ions, molecular models (optional)
Atomic and Periodic Table Basics
1. Which one of the following is matter? Light, air, gravity, heat, neutrons. Explain.
2. Given a periodic table be able to find the alkali, alkali earth, transition, halogens, noble gasses, metalloids, radioactive metals.
3. What is the difference between an isotope and an ion?
4. How do you qualify something as a theory and not a hypothesis?
5. What are the bond angles in the following molecules (Cl2, NH3, H2O, CH4, H2CO)?
Stoichiometry and Reactions
1. Make the following conversions
a) 100.0 g potassium permanganate à moles
b) 100.0 g Iron(III) oxide àmolecules
c) 1.00 x 1012 molecules dinitrogen oxide à moles
d) 100.0 grams NH3 à # protons
e) 1.00 L H2O à # neutrons (hint: 1 g H2O = 1 mL H2O)
2. If 32.5g aqueous silver nitrate reacts with an excess of aqueous copper (II) carbonate,
a) Write out the COMPLETE balanced chemical equation: include the states of matter.
b) Write out the NET IONIC equation.
c) predict how many grams of EACH product should be produced.
3. The combustion of ethyne gas is represented by the equation
_C2H2 (g) + __O2(g) à _CO2 (g) + __ H2O (g)
a. Balance the equation.
b. How many liters of CO2 and grams of H2O are produced when 52.0g C2H2 burns?
c. How many liters of oxygen are required to burn 52.0g of C2H2?
4. What is the percent yield if 4.64g of copper is produced when 1.87g of aluminum reacts with an excess of copper (II) sulfate?
2Al(s) + 3CuSO4(aq) à 1Al2(SO4)3(s) + 3Cu(s)
6. How many grams of SO3 are produced when 20.0g FeS2 reacts with 16.0g O2 according to the balanced equation
4FeS2(s) + 15O2(g) à 1Fe2O3(s) + 8SO3(g)?
a. What is the limiting reagent?
b. What is the excess reagent?
c. If 18.2g SO3 is produced when a student completes this experiment, what is the percent yield?
6. Which is the limiting reagent and which is the excess reagent if 0.48mol P2O5 reacts with 1.52mol H2O in the reaction 2P2O5 + 6H2O à 4H3PO4?
Gas Laws
1. Complete the following conversions:
a. 7.00atm to kPa
b. 202.6kPa to atm
c. 20oC to K
d. 90K to oC
2. What is STP?
3. What is absolute zero? What happens at absolute zero?
4. What are some major differences between solids, liquids and gases? Explain the intermolecular forces.
5. If pressure is held constant, and temperature changes from 27oC to 77oC, what is the final volume if a container starts out at 80.0mL?
6. If a container of gas is held at the same temperature, what is the final volume if it starts out at 200.0mL at 0.350 atm and the pressure is increased to 0.700.0atm?
7. How does a volume change affect the pressure of a gas if the temperature is held constant?
8. How does a pressure change affect the temperature of a gas if the volume is held constant?
9. What is the volume of 1 mole of gas at STP?
10. A gas at 7.75x104Pa and 17oC occupies a volume of 850.0cm3. At what temperature in degrees Celsius, would the gas occupy 720.0cm3 at 8.10x104Pa? (Hint: 1mL = 1cm3)
11. Find the volume, in liters, of an 8.00g sample of O2 held at STP.
12. Calculate the pressure, in atmospheres (atm), exerted by 2.50L HF gas containing 1.35mol at 320.0K.
13. 12. 0.234 moles of argon occupies a volume of 375 mL at a temperature of 25.0°C. Determine the pressure exerted by the gas.
14. Explain the situation(s) where the ideal gas law breaks down.
Solutions and Intermolecular forces
1. What are some of the major properties of water? At least 4.
2. What are some major factors that affect solubility?
3. Describe the dissolving process at the molecular level.
4. What is the difference between a saturated solution, unsaturated solution, and supersaturated solution?
5. Calculate the molarity of a solution which contains 400g CuSO4 in 4.00L of solution. What about a solution containing 0.060mol NaHCO3 in 1500mL of solution?
6. You have the following stock solutions available: 2.00M NaCl, 4.0M KNO3, and 0.50M MgSO4. Calculate the volumes you must dilute to make the following solutions:
a. 500.0mL of 0.500M NaCl
b. 2.0L of 0.30M MgSO4
c. 50.0mL of 0.20M KNO3
7. What is a colligative property? What are some examples?
8. How many grams Ba(NO3)2 are needed to make 2.60 liters of a 1.25 M solution
Chapter 16: Thermochemistry
1. What is the difference between an exothermic process and an endothermic process? Give an example of each. Classify different phase changes as exothermic or endothermic.
2. What is the specific heat capacity of water in calories? Joules?
3. What is the difference between kilojoules and joules?
4. What is the final temperature of a 1 kg copper pipe which started at 25oC, and whose specific heat is 0.385J/g∙C?
5. Using calories, calculate how much heat 32.0g of water absorbs when it is heated from 25.0oC to 80.0oC. How many joules is this?
6. Determine the final temperature of 98g of water at 35ºC when it when it absorbs 2.05kJ of energy.
7. Calculate the specific heat of a 143g rock that goes from 18ºC to 44ºC when it absorbs 3.66 kJ from the sun.
8. What is the standard heat of formation?
9. Calculate the standard heat of formation for
_NH3(g) + O2(g) à _ NO(g) + _H2O(g)
10. What is the second law of thermodynamics?
Organic and Biological Chemistry
1. What are the correct prefixes for hydrocarbon naming in order?
2. List 2-3 special characteristics of carbon that impact how it bonds with elements:
3. Determine the name and formula of the flowing:
4. What is the subunit of protein?
5. Draw the general structure for an amino acid
6. What is a polymer?
7. Draw a diagram that shows the molecular units in DNA (sugar, phosphate, nucleotide, H-bond)
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