Chemistry I

Second Semester Review

The test will cover chapters 10, 12, 14, 16, 19, 20, & 25. There will be 100 multiple choice questions on the test.

Chapter 10: Chemical Quantities: All sections. You should be able to solve any problem involving the

mole.

Chapter 12: All sections in chapter 12. You should be able to calculate stoichiometric quantities from balanced chemical equations, construct mole ratios, identify the limiting reactant, and calculate theoretical and percent yield.

Chapter 14: Concepts in this chapter that you should know are: Kinetic Molecular Theory, Gas Laws and how to calculate, PV=nRT, Dalton’s Law of Partial Pressure, & Graham’s Law. ). Key equations are on pg. 438.

Chapter 17: All sections in this chapter were covered. You should know how to calculate molar heats

using several methods (Hess’s Law and using the standard heats of formation).

Chapter 19: In this chapter we learned how to calculate pH. You should know how to:calculate pH, pOH and the concentrations. Know the six strong acids, the definitions of acids and bases, and identify acid/base conjugate pairs.

Chapter 20: Oxidation and Reduction – oxidation numbers, LEO goes GER, oxidizing and reducting agents. You should also know how to balance Redox reactions.

Chapter 25: In nuclear chemistry you should know the different symbols for the nuclear particles, how to balance a nuclear reaction, be able to identify ionizing radiation, and solve half-life and energy problems.

There will be approximately 14 - 15 multiple choice questions on each chapter. Draw your mole road with the bridge for chapter ten and twelve here:

Chapter Ten: Chemical Quantities

Vocabulary:

  1. molar mass-
  2. mole-
  3. empirical formula-
  4. Avogadro’s hypothesis-
  5. percent composition-

Questions:

  1. Find the molar mass of PCl3, Fe(OH)2, C12H22O11, and Ca3(PO4)2
  2. How many moles are in 0.0688 g of AgCl?
  3. How many grams are in 14.4 moles of F2?
  4. How many atoms in 3.00 mol of Sn?
  5. How many formula units in 0.400 mol of KCl?
  6. What is the volume of 7.6 mol of Ar at STP?
  7. What is the density of Ne at STP?
  8. Determine the empirical formula of a compound with 42.9% C and 57.1% O.
  9. Determine the % composition of each element in N2O3?
  10. How many grams are in 1.8 x 1024 molecules of CF4?

Chapter Twelve: Stoichiometry

Vocabulary:

  1. limiting reactant
  2. actual yield
  3. theoretical yield
  4. percent yield
  5. mole ratio
  6. stoichiometry
  7. excess reactant

Questions:

  1. Calculate the number of moles of potassium chlorate, KClO3, that must decompose to produce KCl and 1.80 moles of oxygen gas. Answer: 1.20 moles
  2. How many moles of oxygen gas are required to burn 34.2 g of CH3OH? The products are carbon dioxide and water. 1.60 mol O2
  1. How many grams of N2H4 are needed to react with 212.3 g of H2O2? The products in the reaction are N2 and water. Answer: 100.0 g
  1. If 15.5 g of aluminum are reacted with 46.7 g of chlorine gas, then aluminum chloride, AlCl3, is formed.
  2. Which reactant is the limiting reactant?
  1. Calculated the number of grams of the excess reactant.
  1. What is the theoretical yield of AlCl3?

d. If 50.0 g of AlCl3 is actually produced, what is the percent yield?

Chapter Fourteen: The Behavior of Gases

Vocabulary:

  1. pressure-
  2. diffusion-
  3. effusion-
  4. ideal gas-
  5. partial pressure-
  6. ideal gas law-

Questions:

  1. A cylinder of nitrogen gas at 25oC and 101.3 kPa is heated to 45oC. What is the new pressure of the gas? Answer: 108 kPa
  1. A gas has a volume of 8.57 L at 273 K. What will be the volume at 355K if its pressure does not change? Answer: 11.1 L
  1. What volume will 24.5 g of carbon dioxide gas occupy at 55oC and a pressure of 88.8 kPa? (17.1 L)
  1. What happens to the pressure of a contained gas in each instance?
  2. More gas particles are added
  3. The temperature of the gas is decreased
  4. The volume of the container is reduced
  1. A gas cylinder has a volume of 6.8 L and is filled with 13.8 g of N2. Calculate the pressure of N2 at 25oC.
  1. The temperature of 1 L of steam at constant volume and 1.00 atm pressure is increased from 100oC to 200oC. What is the new pressure of the steam? Answer: 1.27 atm.
  1. Calculate the following quantities.
  2. The number of liters occupied at STP by 0.620 mol Cl2. Answer: 13.9
  3. The volume of gas at 3 kPa of pressure if the same gas has a volume of 6 L at 0.5 kPa and the temperature is constant. Answer: 1 L
  4. The partial pressure of gas X (Px) in a mixture of three gases, X, Y, and Z if the total pressure (Ptotal) is 50 kPa and the sum of the partial pressures of Y and Z is 30 kPa. Answer: 20 kPa

Thermochemistry

Chapter 17

Vocabulary:

  1. Endothermic
  2. Enthalpy
  3. Exothermic
  4. Heat
  5. Heat capacity
  6. Heat of combustion
  7. Heat of reaction
  8. Hess’s law of summation
  9. Molar head of fusion
  10. Molar heat of vaporization
  11. Specific heat
  12. Standard heat of formation
  13. Thermochemistry

Key Equations: q = mcTmol f =

Practice:

  1. The molar heat of fusion for ethanol is 4.60 kJ/mol. How many kilojoules are required to melt

24.5 g of ethanol at its freezing point? Ans: 2.45 kJ

  1. How much heat, in kJ, must be added to 178 g of water to increase the temperature of the water by 5.0o C? Ans. = 3.7 kJ
  1. Hess’s Law practice #84 on page 537 of your text. Ans = -137 kJ
  1. Using Table 17.4 on page 530 in your text, calculate the molar heat of combustion of methane, CH4. The products are carbon dioxide gas and water vapor. Ans. = -200.6 kJ/mol

Chapter 19: Acids, Bases, and Salts

Vocabulary:

  1. Arrhenius Acid-
  2. Arrhenius Base-
  3. Bronsted Acid-
  4. Bronsted Base-
  5. indicator-
  6. amphoteric-
  7. conjugate acid-
  8. conjugate base-

Questions:

  1. List the formulas and names for the six strong acids.
  1. List the properties of acids and the properties of bases.
  1. Calculate the pH of the following solutions (be sure to take notice whether it is [H+] or [OH-]
  2. 0.005 M HClb. 2.5 x 10-4 M H2SO4c. 3.71 x 10-5 M NaOH
  1. Calculate the [H+] of the for the following: (be sure to take notice whether it is pH or pOH)

a. pH = 2.93b. pH = 10.6c. pOH = 9.87d. pOH = 4.15

  1. List the conjugate acids for the following bases:
  2. NH3b. H2Oc. CO32-
  1. List the conjugate bases for the following acids:
  2. HClb. HSO4-c. H2S

Chapter 20: Oxidation-Reduction Reactions

Vocabulary:

  1. oxidation
  2. reduction
  3. oxidizing agent
  4. reducing agent
  5. oxidation number

Questions:

  1. Assign an oxidation number to each atom in these compounds.
  2. NaNO2
  3. CoSO4
  4. Zn(OH)2
  5. K2PtCl4
  1. Identify these processes as either oxidation or reduction.
  2. Fe3+ + e- → Fe2+
  3. Cr → Cr3+ + 3e-
  4. Cl2 + 2e- → 2 Cl-
  5. Hg → Hg2+ + 2e-
  6. Determine the oxidation number of sulfur in each of the following:
  7. H2Sb. SO2c. Sd. SO42-
  1. Balance the following redox reactions:
  2. Mg + N2 → Mg2+ + N3-
  3. Fe2+ + MnO4- → Fe3+ + Mn2+ (acidic solution)
  4. Cu + NO3- → Cu2+ + NO

Chapter 25: Nuclear Chemistry

Vocabulary

  1. alpha-
  2. beta-
  3. gamma-
  4. half-life-

Questions:

  1. Write the nuclear decay reactions for each of the following.
  2. alpha emission of Ra
  3. beta emission of I
  4. positron emission of K
  5. The radioisotope technetium-99 is often used as a radiotracer to detect disorders of the body. It has a half-life of 6.01 hours. If a patient received a 25.0mg dose of this isotope during a medical procedure, how much would remain 48.0 hours after the dose was given?
  1. Provide the missing term in each of the following equations.
  2. Cf + ______→ 4 n + Sg
  3. ______→He + e
  4. Al + He → Si + ______