You can use the Problem-Set Information Sheet from Chemistry: Problems and Solutions pages 238-243 on your final exam, you may want to write this out in your notes so you have access during the test.
Unit 1 – States of Matter
1. State the definition of each of the following gas laws in words:
a. Boyle’s Law
b. Charles’s Law
c. Gay-Lussac’s Law
d. Ideal Gas Law
What are the assumptions of each of the following laws?
e. Boyle’s Law
f. Charles’s Law
g. Gay-Lussac’s Law
h. Ideal Gas Law
2. What are the equations of each of the following laws?
a. Boyle’s Law
b. Charles’s Law
c. Gay-Lussac’s Law
d. Ideal Gas Law
3. What can you calculate for each of the following laws? And include an example.
a. Boyle’s Law
b. Charles’s Law
c. Gay-Lussac’s Law
d. Ideal Gas Law
4. Increasing the temperature of a 342 cm3 balloon from 278K to 315K, and assuming constant pressure, what is the new volume of the balloon?
5. How many moles of gas are there in a sample in a 15.0 L container at 305 K and 203 kPa? (The gas constant is 8.31 L kPa/mol K).
6. A reaction requires 22.4 L of gas at STP. You have 55.0 L of gas at 100 kPa and 373 K. What is true about this reaction? (The gas constant is 8.31 L kPa/mol K).
7. A 5.0 L container holds a sample of hydrogen gas at 300 K and 100 kPa. If the pressure increases to 350 kPa and the volume remains constant, what will the temperature be?
Unit 2 –Solutions
8. Define the following words, include an example:
a. Solute
b. Solvent
c. Molarity
d. Molality
9. What is the molarity of a 250 mL solution that contains 4.44 g of NaCl?
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10. If 5.86 g of H2SO4 are dissolved in 700 mL of water, what is the molarity of the solution? Use the periodic table.
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Unit 3 – Acids and Bases
11. Draw the pH scale, write down all the numbers & include what is a strong acid, strong base & neutral on the scale.
12. Define the following& be able to identify examples of the following acids and bases:
a. Arrhenius acids
b. Arrhenius bases
c. Bronsted-Lowry acid
d. Bronsted-Lowry base
e. Lewis acid
f. Lewis base
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13. Be able to identify the type of base in various chemical equations.
14. Know the if the following is a strong acid or base or a weak acid or base:
a. Potassium hydroxide
b. Ethyl alcohol
c. Vinegar
d. Ammonia
e. Sodium hydroxide
f. Acetic acid
15. Define pH.
16. Write the equation for pH.
17. A solution has a [H+] concentration of 5.89 x 10-9M. What is the pH?
Unit 4 – Chemical Thermodynamics
18. Define the following:
a. Exothermic reaction
b. Endothermic reaction
c. Calorie
d. Joule
e. Calorimeter
f. Specific heat capacity
19. Give 5 examples of both exothermic and endothermic reactions & explain why each example is categorized this way.
20. What equation do you use to calculate the heat needed to raise the temperature of a substance?
21. How much heat do you need to raise the temperature of 500 g of gasoline from 0°C to 20°C? **hint, use the Specific heat capacity table in lesson 4.06 on slide #4 for the C (J/g°C) of gasoline.
22. A calorimeter contains 350 g of water at 20°C. You place a hand warmer containing 150 g of liquid sodium acetate inside the calorimeter. When the sodium acetate finishes crystallizing, the temperature of the water inside the calorimeter is 39.4°C. The specific heat of water is 4.18 J/g-°C. What is the enthalpy of fusion (?Hf) of the sodium acetate? (Show your work.) Where necessary, use q = mHf.
23. What are the steps to correctly writing a thermochemical equation (Hint – watch the recording from lesson 4.09 if you haven’t already). Write an example of a correctly written thermochemical equation.
Unit 5 – Reaction Rates and Equilibrium
24. Define the following terms:
a. Activation energy
b. Chemical equilibrium
c. Inhibitor
d. Le Chantelier’s Principle
e. Transition state
25. What factors cause reaction rates to increase or decrease? Identify each different situation and what is happening to the collision rates of the molecules.
26. For the reactionCH3CH2OH + 3O2? 2CO2 + 3H2O, ?H = -1,235 kJ/mol at 248 K. What is the ?G, and will this reaction be spontaneous in the forward direction?
Unit 7 – Organic Chemistry
27. Define the following, give examples of each & draw a sketch:
a. Alkane
b. Alkene
c. Alkyene
d. Aldehyde
e. Ether
f. Ester
g. Alkyl halide
h. Amine
i. Alcohol
j. Phenyl
k. Amide
l. Ketone
m. Carboxylic acid
28. Draw a structural formula for 1-hexene (C6H12), which has a double bond between the number 1 and 2 carbons in the chain. What class of compound is it, and what feature distinguishes it as that class?
Unit 8 – Nuclear Chemistry
29. Define the following:
a. Fission
b. Fusion
c. Half-life
d. Isotope
e. Radioactive dating
30. What subatomic particles make up protons? What about neutrons?
31. Calculate the percent of material left each half-life (up to 10 half-lives).
32. If you have 70 g of a substance that decays with a half-life of 24 days, how much do you have left after 280 days?
33. The three major types of radioactive decay of an unstable nucleus are alpha particles, beta particles, and gamma rays.
• Compare and contrast alpha particles, beta particles, and gamma rays.
• Explain how alpha decay works and how it causes transmutations.
• Explain how beta decay works and how it causes transmutations.
• Compare the transmutations caused by alpha and beta emissions.
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