Hoffman Sem 2 Senior Final Review

Chemistry Semester 2 SENIORFinal Exam Study Guide

Name ______

The final exam will be all multiple-choice. Come prepared with a pencil.

Do not bring electronic devices to the exam (other than a calculator). This includes cell phones and mp3 players. If I see them I will take them.

There will be no rest room passes until you are done with the test.

I will provide a formula sheet (identical to one attached to this study guide) and a laminated periodic table.

This study guide will be extra credit toward your final exam grade.

BRING A PENCIL AND A CALCULATOR!!! Don’t come to my final without these.

“Success is a state of mind. If you want success, start thinking of yourself as a success.”

Keys to success:

  • Complete this study guide.
  • Don’t wait until Monday or Tuesday before finals to get help.
  • Start studying early. Remember, you have all summer to relax.
  • Be prepared.

Final exam topics:

  1. Chemical Reactions + Balancing
  2. The Mole + Stoichiometry
  3. Solutions and Solubility
  4. The Gas Laws

Chemical Reactions

Identify and balance each reaction.

1. _____ KClO3  KCl + O2

2. _____ Br2 + NaI  NaBr + I2

3. _____ C2H6 + O2  CO2 +H2O

4. _____ SO3 + H2O  H2SO4

5. _____ Zn +HCl  ZnCl2 + H2

6. List the four signs of a chemical reaction

7. List the four ways to speed up a chemical reaction

8. List the five types of reactions. Explain what happens for each type.

9. Define activation energy and activated complex.

Find the missing values.
For each graph, label the energy of product, energy of reactants, activation energy, activated complex, and change in heat (H).

10.

Energy of reactants
Energy of products / 400
Energy of activated Comp. / 550
Energy of Activation
H Total Heat / 250
Exothermic or Endothermic

11.

Energy Reactants /

600KJ

Energy of Products / 200KJ
Energy of Reaction (ΔH)
Energy of Activation / 300KJ
Energy of Activated Complex
Exothermic or Endothermic

The Mole and Stoichiometry

12) How big is a mole? In other words, what number is equal to a mole?

13) How do you convert from molecules to moles?

14) How do you convert from atoms to moles?

15) How do you convert from atoms or molecules to grams?

16) How many moles are in 3.54x1024 atoms of Cu?

17) How many molecules are in 8.7 moles of Ne?

18) How many moles of S8 are in 12.3x1025 molecules of S8?

19) How many moles are there in 150 grams of Al(OH)3?

20) How many moles are there in 68 grams of CuSO4?

21) How many grams are there in 4.4 moles of Fe2(SO4)3?

CO2 + LiOH  Li2CO3 + H2O

22) Balance the previous equation

23) How many moles of CO2 react to form 5.4 moles of Li2CO3?

24) How many moles of CO2 react to form 2.8 moles of H2O?

25) How many moles of LiOH react to form 9.2 moles of Li2CO3?

MgCl2 + AgNO3 --> Mg(NO3)2 + AgCl

26) Balance theprevious equation.
27) Howmany moles of Mg(NO3)2areformedwhen 76.2grams of AgNO3react?

28) Howmany grams of AgCl areformedwhen 293.3grams of Mg(NO3)2react?
29)How many grams of MgCl2 are needed to produce 138.7 grams of Mg(NO3)2?

Given the balanced equation, answer the two questions that follow.

2 Zn (s) + O2(g)  2 ZnO (s)

30) Calculate the mass of product that can be produced from 2.36g of zinc metal.

31) How many grams of oxygen gas must react to give 1.28g of ZnO?

Given the balanced equation, answer the two questions that follow.

2 Bi(s) + 3 Cl2(g)  2 BiCl3(s)

32) Calculate the mass of product that can be prepared from 5.6g of bismuth metal.

33) How many grams of chlorine gas must react to give 35.2 g of BiCl3?

Given the equation, answer the two questions that follow. (Is the equation balanced?)

Cu(s) + AgNO3(aq)  Cu(NO3)2(aq) + Ag(s)

34) What is the mass of silver that can be prepared from 0.825g of copper metal?

35) How many grams of silver nitrate must react to give 3.00g Ag?

Given the equation, answer the two questions that follow. (is the equation balanced?)

Co + HgCl2  CoCl3 + Hg

36)What is the mass of mercury that can be prepared from 2.35g of cobalt metal?

37) How many grams of mercuric chloride must react to give 5.35g Hg?

Given the equation, answer the two questions that follow. (is the equation balanced?)

Na3PO4(aq) + Ca(OH)2(aq)  Ca3(PO4)2(s) + NaOH(aq)

38) What is the mass of calcium phosphate that can be prepared from 1.78g of Na3PO4?

39) How many grams of calcium hydroxide must react to give 2.39g of Ca3(PO4)2?

40) Mustard gas, C4H8SCl2, has been used as a weapon in chemical warfare. Find the percent composition of each element in mustard gas.

41) What is the percentage of carbon in propane (gas grill fuel), C3H8?

42) A fire extinguisher uses carbon dioxide gas (44 g/mol) to smother a fire. A particular fire extinguisher releases 1.45 L of CO2 gas at STP. What is the mass of the CO2 gas that was released?

43) The main ingredient of the self-defense agent MACE is chloroacetophenone, C6H5COCH2Cl. This compound is prepared by chlorination of acetophenone, C6H5COCH3.

C6H5COCH3 + Cl2  C6H5COCH2Cl + HCl

What mass of chloroacetophenone would be produced by the reaction of 4.00 g of acetophenone with 10.4 g of chlorine? What is the limiting reactant? Which reactant is in excess and by how many grams is it in excess?

Solutions and Solubility (Molarity)

Calculate the molarity for each of the following solutions.
BE SURE GRAMS ARE CONVERTED TO MOLES and mL INTO LITERS

59)2.50 g NaCl in 100.0 mL of solution

60) 3.60 g K2Cr2O7 in 100.0 mL of solution

What volume of each of the following solutions contains the indicated amount of dissolved solute?
BE SURE GRAMS ARE CONVERTED TO MOLES and mL INTO LITERS

61) 10.0 g solute in 1.27 M NaF

62) 10.0g solute in 2.40 M K2CO3

What is the mass of solute dissolved in the indicated volume of each of the following solutions?

63) 1.00 L of 0.250 M NaOH

64) 250.0 mL of 0.500 M CuCl2

65) What is the molarity of a saturated solution of calcium sulfate that contains 0.64 g of solute in 100 mL of solution?

66) A hospital glucose solution is analyzed to verify its concentration. A 10.0 mL sample with a mass of 11.48 g is evaporated to dryness. If the solid glucose residue has a mass of 0.425 g, what is the molarity of the glucose, C6H12O6, solution?

Use the solubility curve to answer questions 67-73

67) at 30oC, which salt is least soluble?

68) at 100oC, which salt is more soluble, potassium chloride or potassium chlorate?

69) if 8g of potassium chlorate are added to 100g of water at 10oC, how many grams do not dissolve?

70) if all 45g of KCl were dissolved in 100mL of water at 70oC, the solution would be saturated, unsaturated, or supersaturated?

71) What mass of ammonium chloride would be needed to make a saturated solution at 80oC?

72) Which substance(s) on the solubility curve do you think are gases? Why?

73) What type of solution occurs at 70oC when 55g of KCl is dissolved to 100g of water?

Use the solubility curve to answer questions 74-77

74) At 45oC, how many grams of potassium nitrate would dissolve in 300g of water?

75) If a saturated solution at 20oC contained 20g of ammonia, how much water is present?

76) If you put 20g of potassium nitrate into 200g of water at 10oC, what type of solution do you have?

77) How many grams of water would it take to dissolve 65g of NaCl at 40oC?

Decide if the questions 78-82 describe an unsaturated, saturated, or supersaturated solution.

78) A solution is prepared by adding 30g of KCl to 100g of water at 50oC.

79) A student adds 30g of NaCl to 100g of water at 80oC.

80) A label on a flask reads 10g KClO3 / 100g H2O. A thermometer indicates the temperature of the solution to be 25oC. No crystals are visible in the bottom of the flask. The solution must be ______solution?

81) If you drop a crystal into a beaker of sodium acetate and crystals immediately form and fill the beaker.

82) The maximum amount of solute is dissolved in 100g of water.

83) Define solute.

84) Define solution.

85) Define solvent.

86) What are three ways of speeding up the rate at which a solid dissolves?

a.

b.

c.

87) How can solubility of a gas be increased when dissolved in a liquid?

88) What type of mixture is a solution? (circle your answer)

homogenous or heterogenous

89) You have a solution that has 15g of sugar dissolved on 100g of water.

  • What is the solute? ______
  • What is the solvent? ______

The Gas Laws

90) A 75.0 cm3 sample of fluorine gas at 15oC has a pressure of 761 torr. If the gas is heated to 100oC at 761 torr, what is the final volume in cubic centimeters?

91) Calculate the final Celsius temperature of sulfur dioxide if 0.550 L of the gas at 45oC and 560 mm Hg is heated until the pressure reaches 754 mm Hg. Assume the volume remains 0.550 L.

92) If a sample of gas occupies 125.0 mL at –25oC and 740 mm Hg, what is the volume at 25oC and 350 mm Hg?

94) Draw and label a graph to represent Boyle’s Law, Charles’ Law, and Gay-Lussac’s Law.

95) State Boyle’s Law, Charles’ Law and Gay-Lussac’s Law.

Boyle’s:

Charles’

Gay-Lussac’s

96) If a container has 30 moles of O2 and is at a temperature of 15oC and a pressure of 745 torr, how many liters is this container?

97) A container has 105 L of CO2 and is at a temperature of 110oC and a pressure of 60 atm. You transfer the gas to a container with 0.8 L and a pressure of 100 atm. What is the new temperature in degrees Celsius (oC)?

98) What is the resulting pressure when you transfer gas from a cylinder with a temperature of 22oC and a pressure of 4 atm into a container with a temperature of 65oC? Assume volume remains constant.

99) You pulled a tank of pressurized air out of storage. This tank was in a hot storage building with a temperature of 75oC. The tank’s pressure gauge reads 2,500 psi and its volume is 35 ft3. You then take the air and put it into a different cylinder with a volume of 15 ft3 and a pressure of 2,000 psi. What will be the new temperature of the tank?

100) Calculate the new volume of chlorine gas at 15oC and 75.0 cm Hg if the volume of the gas is 1.10L at 23oC and 85.5 cm Hg.

101) Calculate the final Celsius temperature of hydrogen chloride gas if 1.50 L at 46oC and 0.750 atm is heated until the volume reaches 1.26 L at 0.750 atm.

Miscellaneous

Use the equation below to answer the following questions 101-107

(Is it balanced? You didn’t even need to read this sentence because you already knew to check)

Cu(NO3)2 (aq) + Na2CO3 (aq)  CuCO3(s) + NaNO3 (aq)

102) I have 6.7 moles of Na2CO3. How many molecules is that?

103) What is the molar mass of each reactant?

Cu(NO3)2

Na2CO3

104) How many grams are in 6.7 moles of sodium carbonate?

105) How many moles of copper(II) nitrate react with sodium carbonate to form 1.8 moles of sodium nitrate?

106) How many grams of copper (II) nitrate react with sodium carbonate to form 1.8 moles of sodium nitrate?

107)How many grams of sodium carbonate react with copper (II) nitrate to form 1.8 moles of sodium nitrate?

108) Calculate the mass of copper (II) carbonate that can be produced from the reaction of 2.36 g of copper (II) nitrate with sodium carbonate.

Formula Page- The same one you will get the day of the final exam

Avogadro’s # = 6.02 x 1023

P1V1=P2V2V1/T1=V2/T2

P1/T1=P2/T2

PV=nRT R=0.0821 atm*L/mol*K

(oF-32) x 5/9 = oC (oC x 9/5) + 32= oF

Celsius to Kelvin: oC + 273 Kelvin to Celsius: K – 273

Molarity equation
(YES they must be moles or liters. Be sure to convert numbers to match units!)

(Activation energy) = (Activated complex) - (Energy of Reactants)

(Energy of Reactants) + (Change in heat) = (Energy of products)

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