Chemistry Chapter 9 Test Review
Chemistry Final EXAM Review Chapters 9-16
& Chemistry MATH REVIEW
Chemistry Chapter 9 Test Review
1. Describe a chemical reaction.
2. Define reactant.
3. Define product.
4. Identify the products and reactants in a reaction.
5. Identify a chemical change.
6. Relate the symbols in a chemical equation to the words in a word equation.
7. Write the word equation from a sentence.
8. Write a formula equation from a word equation.
9. Describe a balanced equation.
10. Compare the mass of reactants to the mass of products.
11. Describe the meaning of coefficients in a chemical equation.
12. Identify the number of atoms of an element that are present in a chemical equation.
13. Describe the allowed steps in balancing a chemical equation.
14. Identify the state symbols used in a chemical equation.
15. Interpret the state symbols used in chemical reactions.
16. Balance a chemical equation.
17. Define the reaction types.
18. Identify the general forms of the reaction types.
19. Identify the type of reaction from its chemical equation.
20. Describe the activity series.
21. Use the activity series to determine the result when metallic solutions are mixed.
22. Write a sentence equation for a reaction.
23. Write a formula equation for a reaction.
24. Balance a chemical equation.
Chemistry Chapter 10 Test Review
1. What are the units for atomic mass?
2. Define formula mass.
3. How is the number of atoms related to mass and atomic mass?
4. Define mole (related to carbon-12).
5. Identify a diatomic molecule.
6. What is a formula unit used for?
7. What is Avogadro’s number?
8. What is the symbol for Avogadro’s number?
9. Define molar mass.
10. What are the units for molar mass?
11. What is the symbol for molar mass?
12. Relate volume to number of molecules for equal temp and pressure.
13. Define standard temperature.
14. Define standard pressure.
15. Identify the molar volume for a gas at STP.
16. Relate volume to other characteristics of a gas.
17. Define percentage composition.
18. Determine the sum of percentage compositions.
19. Find the percentage composition of a substance.
20. Define empirical formula.
21. Define molecular formula.
22. State the empirical formula of a substance.
23. Find the empirical formula from the molecular formula.
24. Find the molecular formula from the empirical formula.
25. Find the number of atoms in a given number of molecules.
26. Find the mass of a given number of molecules.
27. Find the formula mass for a substance.
28. Find the molar mass of a substance.
29. Given the number of grams of each atom, find the empirical formula. Given additionally the molar mass, determine the molecular formula.
30. Determine the percentage composition for a substance given the total and element masses.
Chemistry Chapter 11 Test Review
1. Define stoichiometry.
2. What does stoichiometry do for you?
3. How is the molar ratio determined?
4. What do coefficients represent?
5. In a mass-mass problem, mass is first converted to what?
6. How is number of moles found from mass and molar mass?
7. What are the general steps (conversions) for a mass-mass problem?
8. When talking about moles of a substance we really mean what?
9. What type of stoichiometry problem is essential for all the rest?
10. What is the first step in a stoichiometry problem?
11. What conditions are necessary for any volume problem?
12. The factor to convert volume to moles has what value?
13. How is the molar volume used to convert moles of a gas to volume?
14. When the reactants are in stoichiometric proportions, what happens?
15. How much limiting reactant is left after a reaction?
16. How much excess reactant is left after a reaction?
17. What does the limiting reactant determine?
18. How do you find which reactant is limiting given a balanced equation?
19. Define expected yield.
20. Define percent yield.
21. Find the expected ratio of gas volumes in a reaction.
22. Compare numbers of particles based on a balanced equation.
23. Use a balanced equation to find the volume produced given the initial volume.
24. Use a balanced equation to find the mass of product given the volume of reactant.
25. Do a moles-mass problem.
26. Do a mass-moles problem.
27. Do a mass-mass problem
28. Do a mass-volume problem.
29. Do a limiting reactant problem and then find percent yield.
30. Do a limiting reactant problem.
Chemistry Chapter 12 Test Review
1. Discuss energy requirements for bond breaking and formation
2. Define thermochemistry
3. Describe exothermic reactions
4. Describe endothermic reactions
5. Where is heat term for exothermic reaction?
6. Where is heat term for endothermic reaction?
7. Define enthalpy change
8. State conditions for enthalpy change
9. State the physical condition of an element for a reaction under standard conditions
10. Define Hess’s law
11. Discuss changes to ΔH for a change to chemical equation
12. Discuss changes to ΔH for a change to chemical equation
13. Identify a type of enthalpy change (a heat)
14. Define calorimetry
15. Define heat capacity
16. Define specific heat
17. Define heat
18. Find the enthalpy of reactant from an enthalpy diagram
19. Find the enthalpy of product from an enthalpy diagram
20. Find the enthalpy change for a reaction from an enthalpy diagram
21. Classify reactions from enthalpy diagram as endo- or exo-thermic
22. Find ΔHo for a reaction given some equations and ΔH’s
23. Find ΔHo for a reaction given some equations and ΔH’s
24. Find the temperature change of water for a calorimeter reaction
25. Find qsur for a calorimeter reaction
26. Find qrxn for a calorimeter reaction
27. Given a balanced equation with heat term, find the quantity of heat transferred for a given mass reacting
28. Do a Hess’s law problem
29. Find the amount of heat transferred to water given Ti, Tf, and volume
30. Calculate enthalpy change per mole given sentence equation, moles of reactant, amount of water and temperature change of water in calorimeter.
Chemistry Chapter 13 Test Review
1. What is air composed of?
2. What properties do all gases have in common?
3. What is the most important idea for the gas model?
4. Describe the particles that make up gases
5. Identify gas properties
6. Describe the result of changing temperature of gas in a fixed volume
7. Describe perfectly elastic collisions between gas particles
8. State the reason gases spread rapidly through other gases
9. State the reason gases don’t condense unless the temperature is lowered
10. Identify the variables needed to describe a gas
11. Identify the unit that describes the amount of gas present
12. Identify the instrument used to measure gas pressure
13. For constant amount and temperature of a gas, relate pressure and volume
14. For a sample of gas at constant pressure, relate volume and temperature
15. Identify the temperature scale that has absolute zero
16. For constant temp, pressure and volume for two gases, relate number of particles
17. Identify scientist famous for work on partial pressure
18. State the law of partial pressure
19. State conditions for a real gas to behave ideally
20. Identify the temperature scale used in the ideal gas equation
21. Identify the units of R, the ideal gas constant
22. Discuss effects of increased temperature and pressure on the walls of a container
23. Identify the two simplifying, but false assumptions of the ideal gas law
24. Indicate how to make a balloon rise in air
25. How is density related to temperature and volume?
26. Identify the factor that leads to the lifting power of gases
27. Identify the gas that has the greatest lifting power from choices
28. Convert gas pressure units
29. Find the new volume for a balloon given Vi, Ti, and Tf
30. Find the number of moles of a gas given V, P, and T
Chemistry Chapter 14 Test Review
1. State reason for the term “condensed states of matter” for liquids and solids
2. Compare properties of liquid particles to gas particles
3. State reason for greater compressibility of gas particles
4. Identify distinguishing characteristic for solids and liquids
5. List states of matter according to disorder
6. Identify the factor that determines state of matter at a given temperature
7. Relate temperature to kinetic energy of particles
8. Relate type of bonds to physical state
9. Identify particles in a molecular substance that experience bonds
10. Identify property resulting from strong intermolecular forces
11. Compare strength of intermolecular forces to intramolecular forces
12. Define dispersion force
13. Discuss the strength of induced dipole attractions
14. Identify the type of atoms affected by dipole-dipole forces
15. List the atoms that form hydrogen bonds
16. State affect of hydrogen bonding on boiling point of water
17. Relate strength of forces to viscosity
18. Relate strength of forces to surface tension
19. Identify most important difference between solids and liquids
20. Define unit cell
21. Describe hydrates
22. Give another name for amorphous solids
23. Identify types of crystalline solids
24. Identify the characteristic feature of metals
25. Identify type of crystalline solid that has highest melting point
26. Relate change in physical state to change in energy
27. Describe the kinetic energies of particles at a given temperature
28. Define dynamic equilibrium
29. Use a phase diagram to determine change in vapor pressure with change in IMF
30. Use a phase diagram to determine boiling point for a given pressure.
Chemistry Chapter 15 Test Review
1. Identify properties of solutions
2. Discuss the solute particles in a solution
3. Define alloy
4. Identify examples of solutions
5. Define aqueous solutions
6. Define molarity
7. Define molality
8. Define mole fraction
9. Identify factors necessary for finding molality
10. Identify factors necessary for finding molarity
11. Define saturated
12. Define supersaturated
13. Discuss energy needs to form a solution
14. Identify when energy is given off in solution formation
15. Discuss how solution formation can be exothermic
16. Identify factors influencing solubility
17. Identify substance that would dissolve an ionic substance the best
18. Identify the substance that has solubility affected by pressure
19. Identify factors that affect the extent to which a solute dissolves
20. Identify method for preparation of supersaturated solution
21. Identify factors that affect the rate at which a solute dissolves
22. Identify colligative properties
23. Identify factor affecting colligative properties
24. Identify concentration unit used in calculating colligative properties
25. Discuss the change in boiling point of a solution
26. Calculate moles of solute to lower freezing point given ΔT, kf and mass
27. Calculate molality given ΔT and kb
28. Calculate freezing point given kf, molality, and freezing temperature
29. Calculate the boiling point given kb, boiling temperature, and molality
30. Calculate the molarity given mass of substance and volume of solution
Chemistry Chapter 16 Test Review
1. Define chemical equilibrium
2. Define reversible reaction
3. Identify the symbol for a reversible reaction
4. State the relationship between concentration and rate
5. Identify the symbol for concentration
6. Describe the relationship between concentration of reactants and products at equilibrium
7. Identify the scientist that formulated the law of mass action
8. Describe the law of mass action
9. Identify a generic equilibrium constant
10. Identify the symbol for equilibrium constant
11. Define the law of chemical equilibrium
12. List the factors influencing the equilibrium constant
13. Describe "equilibrium lies to the right"
14. Discuss the value of Keq based on the direction of a reaction
15. Discuss the result when Keq ≈ 1
16. Define homogeneous equilibrium
17. Identify the symbol for reaction quotient
18. Describe the use of the reaction quotient
19. Compare the values of Keq and Q at equilibrium
20. Define Le Chatelier's principle
21. Discuss the equilibrium position when conditions at equilibrium are changed
22. Discuss the result of adding reactant to a system at equilibrium
23. Identify a factor that will change the equilibrium constant
24. Write an equilibrium expression for a given reaction
25. Calculate the concentration given the reaction, Keq, and some concentrations
26. Calculate the equilibrium constant given reaction and concentrations
27. Calculate Q and if not in equilibrium, state direction of shift
28. Given an equation, determine the direction of shift if a substance is added
29. Given an equation, determine the direction of shift if a substance is removed
30. Given an equation, determine the direction of shift if pressure and temperature are changed
Chemistry Final Exam Math Review
1. Know how to write a word equation & formula equation.
2. Be able to balance a chemical equation.
3. State the type of chemical reaction.
4. Determine the number of atom in a specific number of grams of a compound.
5. Determine the volume of a gas, given an amount of moles of the gas.
6. Calculate a mass to mass problem
7. Calculate an enthalpy problem.
8. Convert units of pressure.
9. Calculate a Boyle’s Law problem.
10. Calculate a Charles’ Law problem.
11. Calculate a Dalton’s Law problem.
12. Calculate an Ideal Gas Law problem
13. Determine the molarity of a solution.
14. Determine the molality of a solution.
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