Download Semester II Exam Review Questions

Semester II Exam Review Questions
Chapters:
7, 8, 9, 10, 11, 12.4, 13, and 15
Name the following Ionic Compounds
1. MgCl2
__________________________
2. FeO
__________________________
3. Na3PO4
__________________________
4. Co3N2
__________________________
5. AlF3
__________________________
6. Cu(OH)2
__________________________
7. CaCO3
__________________________
8. Pb(NO3)2
__________________________
Write the formula for the following ionic compounds
1. Nickel (II) Chlorate
__________________________
2. Sodium Iodide
__________________________
3. Gallium Phosphide
__________________________
4. Strontium Sulfite
__________________________
5. Tin (IV) Oxide
__________________________
6. Vanadium (V) Nitride
__________________________
7. Zinc oxalate
__________________________
8. Chromium (III) Phosphite __________________________
Name the following binary non-metal compounds.
1. PBr3 ________________________________
2. CO
________________________________
3. N2O4 ________________________________
4. CCl4 ________________________________
5. SiO2 ________________________________
6. BCl3 ________________________________
7. CS2 ________________________________
8. S2Cl2 ________________________________
Write formulas for the following binary non-metal compounds.
1. phosphorus pentachloride
________________________________
2. oxygen difluoride
________________________________
3. sulfur trioxide
________________________________
4. dinitrogen pentoxide
________________________________
5. silicon tetrabromide
________________________________
6. carbon dioxide
________________________________
7. boron triiodide
________________________________
8. sulfur hexafluoride
________________________________
Name the following acids.
1. H2SO3
____________________________________________
2. HNO3
____________________________________________
3. HIO4
____________________________________________
4. HF
____________________________________________
5. H2SO4
____________________________________________
6. H3PO3
____________________________________________
7. HC2H3O2
____________________________________________
8. HClO
____________________________________________
Write formulas for the following acids.
1. nitrous acid
___________________
2. phosphoric acid
___________________
3. bromic acid
___________________
4. hydroiodic acid
___________________
5. hypobromous acid
___________________
6. oxalic acid
___________________
7. perchloric acid
___________________
8. hydrosulfuric acid
___________________
Classifying, Finishing and Balancing reactions
Balance the following equations and indicate the type of reaction taking place:
1. ____________________
2. ____________________
____ Ba + ____ N2  ____ Ba3N2
____ Ca(OH)2 + ____ Al2(SO4)3  ____ CaSO4 + ____ Al(OH)3
3. ____________________
____ K + ____ Fe2O3  ____ Fe + ____ K2O
4.
____________________
____ C6H14 + ____ O2  ____ CO2 + ____ H2O
5.
____________________
____ PbSO4  ____ PbO + ____ O2 + ____SO2
Classify, complete, and balance each of the following chemical equations.
6. Aqueous Calcium hydroxide combines with aqueous ammonium chloride, forming aqueous Ammonium
hydroxide and aqueous Calcium Chloride.
7. Solid Sodium is combined with aqueous Zinc Iodide, forming aqueous Sodium Iodide and solid Zinc.
8. Solid Aluminum combines with gaseous chlorine, forming solid Aluminum chloride.
9. Solid Zinc and aqueous lead (II) nitrate react to form aqueous zinc nitrate and solid lead.
10. Aqueous sodium phosphate and liquid water are formed when aqueous sodium hydroxide reacts with
phosphoric acid.
Chemistry I: Semester Review Questions – The Mole and Stoichiometry
1. How many particles of CO2 are present in 245 g of CO2
2. How many liters of oxygen gas at STP are required to react with 65.3 g of aluminum in the production
of aluminum oxide? Write and balance the reaction first.
3. Copper reacts with silver nitrate to form silver and copper(II) nitrate. How many grams of copper are
required to react with 50.0 mL of 8.0M AgNO3? Write and Balance the reaction first.
4. A substance is found to be composed of 70.58% Carbon, 5.93% Hydrogen, and 23.49% Oxygen. Find
the empirical formula for the substance.
Empirical Formula ____________________
5. Given that the substance above has a molar mass of 204.24 g/mole, find the molecular formula of the
substance. Show your work.
Molecular formula:
6. Zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas. How many liters of 3.75
M HCl are needed to fully react with 165.53 g of zinc? Write and Balance the reaction first.
7. For ZnCl2, calculate the Percent Composition of each element.
Data Table: The Reaction between Tin(II) Nitrate and Aluminum
Mass of Empty Beaker
Mass of beaker and Tin (II) Nitrate
Trial 1
34.56 g
78.84 g
Mass of Aluminum metal
6.45 g
Mass of beaker and Tin (Sn) Metal after reaction
64.76 g
1. Balance the following Equation:
_____ Sn(NO3)2
+
_____ Al

_____ Al(NO3)3
+
_____ Sn
2. Determine the Mass of Aluminum metal and Tin(II) Nitrate used in this reaction.
3. Using the information from question (2) (the masses) and the balanced equation, calculate the theoretical
amount of Tin (Sn) that should have been produced from this reaction. (hint: determine the limiting
reactant)
Theoretical yield =_________________________, Limiting reactant = ______________
4. Using the above data table, calculate the actual amount of Tin (Sn) produced from the reaction.
5. Using the information from questions 3 & 4, calculate the percent yield of Tin for the reaction.
Based on your answer to #3 (the limiting reactant), find out how much of the excess reactant should be left at
the end of the experiment.
Chemistry I: Semester Review 12.4 and 15
1. List the 6 phase changes that can happen with matter. Circle the ones that are endothermic (that have to
GAIN heat to make the change). Put a star by the changes that create more bonds.
__________________________
_________________________
__________________
__________________________
_________________________
__________________
2. During a phase change, the temperature does not increase, but there is a change in the amount of energy.
Explain where that energy goes.
Use the diagram for the element “Malack” below to answer the questions. If a question asks for a
“region”, answer by giving the appropriate letter or letters.
3. In what region(s) is the temperature
increasing?
M
I
H
G
E
4. In what region(s) is the temperature constant?
5. In what region(s) would vaporization occur?
6. In what region(s) would freezing occur?
7. If sublimation were to occur, the element
would jump from what region to what region?
8. A certain number of grams of Malack has 40
Joules of energy and they are at a temperature of
80 oC.
A). What can you say for sure about the Malack? What phase(s) could it be?
B). If 160 J of energy is added to the Malack, give the final temperature and phase of the Malack.
9. A certain number of grams of Malack is at 180 kJ of energy and a temperature of 280 oC. If this sample of
Malack releases 110 kJ of energy, what phase change will the Malack go through?
Use the diagram on the left to complete the
activities and questions about the element
“Yummygum”.
10. Label the regions of the diagram that
correspond to the solid, liquid, and vapor
phases. (Write the name of each phase
directly on the graph in the appropriate
regions).
11. Put a star on the point that represents the
critical point for Yummygum.
A). What temperature is the critical point at?
B). What does it mean to be the critical point? What happens at this point?
12. Put a big circle around the triple point for Yummygum.
A). What are the temperature and pressure for the triple point?
B). What does it mean to be the triple point? What happens at this point?
13. What is the boiling point temperature for Yummygum when the external pressure is 75 atmospheres?
14. What is the freezing point temperature for Yummygum when the external pressure is 70 atmospheres?
15. If you were to have a container of Yummygum in your kitchen, in what state (phase of matter) would you
expect it to be? Explain your answer.
16. A container of Yummygum is sitting at a pressure of 45 atm and temperature of 100 oC. What will happen
as the temperature is increased 400 oC?
17. A container of Yummygum is sitting at a temperature of 100 oC and 1 atm of pressure. What phase change
will occur if the pressure is increased to 90 atm?
18. Why can Yummygum not be brought to boil at a temperature of 200 oC?
19. If it is not poisonous, could Yummygum be used as a drink on earth? Explain your answer.
Show work and the proper units and significance on all problems.
20. How much heat is required to warm 125 g of water from 15.0 to 47.0 oC?
21. What is the specific heat of a metal if the temperature of a 12.5-g sample increases from 19.5 oC to 33.6 oC
when it absorbs 37.7 J of heat?
22. The temperature of 55.6 g of a material changes from 35.0 oC to 20.2 oC when it loses 3080 J of heat. What
is its specific heat?
23. Calculate the amount of heat released, in joules, as 65.0 g of steam cools from 175 oC to -25 oC. Create a
heating or cooling curve to represent the overall change.
24. A candy bar has a total mass of 75.0 grams. In a calorimetry experiment, a 2.76-g sample of this candy bar
was burned in a calorimeter surrounded by 500.0 g of water. The temperature of the water in contact with the
burning candy bar was measured and found to increase from an initial temperature of 22.3oC to a final
temperature of 31.2oC.
a. Calculate the amount of heat in calories released when the 2.76-g sample burned.
b. Convert the heat in calories to nutritional Calories and then calculate the energy content (fuel
value) in Cal/g.
c. Calculate the total caloric content of the candy bar in Calories.
____ C10H22 + ____ O2  ____ CO2 + ____ H2O + 13483kJ
1. What volume of CO2 is produced when 45610 kJ are released at STP?
2. How many kJ’s of energy are produced when 67.5 grams of C10H22 is completely combusted?
3. 50.0 grams of C10H22 and 711 grams of O2 are reacted. Determine the theoretical yield of energy for
this reaction.
4. Using the limiting reactant, determine the number of grams of excess reactant leftover at the end of the
reaction.
Chemistry I: Gas laws Semester Review Questions
FOR EACH OF THE FOLLOWING, NAME THE GAS LAW AND SOLVE THE PROBLEM:
1. How many moles of chloroform, CHCl3, are required to fill a 253-mL flask at 100.0C and 1.26 atm?
2. You want the pressure inside a bottle to be 75.0 kPa at 23C. At what temperature in Celsius should you
seal the bottle when the pressure is 112.5 kPa?
3. A diver’s lungs hold about 20.0 L of air underwater at a pressure of 875 mm Hg. Assuming he holds his
breath and his lungs don’t burst, what will be the volume of air in his lungs at standard pressure on the
water’s surface?
4. What pressure is required to compress a gas that occupies 6500 L at 25C and 1.0 atm to a volume of 40.0 L
at 18C?
5. What is the temperature of a 0.00893 mol sample of neon gas that has a volume of 0.302 L and a pressure of
0.941 atm?
6. A gas occupies 4.78 L at 78.1 kPa and 25C. What will the volume be at 95.7 kPa and 15C?
7. A shampoo bottle contains 443 mL of air at 65C. What is its volume when it cools to 22C?
Use the data table and reaction below to answer the following questions.
Mass of Magnesium (grams)
0.0362 g
Temperature of Water and Hydrogen gas
Volume of Hydrogen
Barometric Pressure
Vapor Pressure of Water at 21.0 oC
21.0 oC
36.1 mL
750.57 mmHg
18.7 mmHg
_____ Mg + _____ HCl  _____ H2 + _____ MgCl2
1. Balance the reaction above.
2. Calculate the moles of Hydrogen produced.
3. Calculate the partial pressure of Hydrogen using Dalton’s Law.
4. Convert mL of hydrogen gas to L of Hydrogen gas.
5. Convert Temperature to Kelvin.
6. Calculate the Ideal Gas Law Constant “R” using the Ideal Gas Law.
7. Using the combined gas law convert the volume of Hydrogen gas collected for STP conditions.
8. Use the corrected volume of Hydrogen gas and the moles to calculate the molar volume of gas at STP.
REMEMBER: 1cm 3 = 1 mL & 1 dm3 = 1 L
Laws:
P1V1T2 = P2V2T1
Ptotal = P1 + P2 + …
PV = nRT
R = 0.0821
atm  L
KPa  L
or R = 8.31
mol  K
mol  K