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Test your basic knowledge |
CLEP Chemistry 1
Start Test
Study First
Subjects
:
clep
,
science
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can
study here
.
Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.
This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.
1. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
activation energy barrier (Le Chatelier's principle)
boiling point
10 degrees
limiting law
2. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.
boiling point
Raoults law
titration
third law of thermodynamics
3. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
negative
boiling point elevation
second law of thermodynamics
Van der Waals
4. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
positive
irreversible and reversible processes
decreases
heats of formation
5. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
equation of state
bohr model
colligative property law
second law of thermodynamics
6. The heat required to change 1mole of solid completely to vapor.
freezing point depression
adiabatic process (thermodynamics)
isopiestic process (thermodynamics)
molar heat of sublimation
7. The temperature at which a substance's solid and liquid phases are in equilibrium.
point particles
entropy
saturated solution
melting point
8. State ________ depend only on the present state of the substance and not on the path by which the present state was attained. Enthalpy - energy - Gibbs free energy - and entropy are examples.
pressure
end point
state functions (thermodynamics)
positive charge
9. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.
double replacement/displacement
limiting law
metallic
reversible
10. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.
kinetic molecular theory
Nernst equation
...
vapor pressure
11. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
molar heat of sublimation
pi bonds
heats of formation
12. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
moles (Le Chatelier's principle)
hybridyzation
Raoults law
electrolytic reactions
13. A state function in which it is the heat content of a substance.
hybridyzation
enthalpy
...
isopiestic process (thermodynamics)
14. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.
equilibrium
electronegativity
equivalent point
cathode rays
15. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).
molar heat of sublimation
state (thermodynamics)
base - acid
Van der Waals
16. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
Charles law
upper right corner
isopiestic process (thermodynamics)
decreases
17. The law stating that change in internal energy is equal to the difference between the energy supplied toi the system as heat and the energy removed from the system as work performed on the surroundings.
partial
first law of thermodynamics
Le Chatelier's principle
kinetic molecular theory
18. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
absorbs (in atomic spectra)
electrolytic reactions
specific heat
left (Le Chatelier's principle)
19. In an endothermic process - energy is absorbed and ^E is _______.
increasing
total pressure (Le Chatelier's principle)
Le Chatelier's principle
positive
20. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
isothermal process (thermodynamics)
zero
positive
first law of thermodynamics
21. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
irreversible and reversible processes
activation energy
electronegativity
decreases
22. In an exothermic process - energy is released and ^E of reaction is ________.
total pressure (Le Chatelier's principle)
negative
emits (in atomic spectra)
end point
23. Electronegativities ________ from left to right in a period.
Avogrados law
increases
boiling point
Charles law
24. The heat change during a process carried out at a constant pressure.
end point
change in enthalpy
isothermal process (thermodynamics)
activation energy barrier (Le Chatelier's principle)
25. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.
...
Valence Shell Electron Pair Repulsion (VSEPR)
base - acid
negative
26. The freezing point - boiling point - and vapor pressure of a solution differ from those of the pure solvent by amounts which are directly proportional to the molal concentration of the solute.
saturated solution
colligative property law
Le Chatelier's principle
ionization energy
27. Metals have electronegativities less than ____
electrolytic reactions
entropy
2
sublimation
28. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
metallic
negative
dynamic equilibrium
point particles
29. In titration - this is the point at which a particular indicator changes color.
end point
double replacement/displacement
...
catalysts
30. The _____ speed up the rate of a chemical reaction but do not change the equilibrium constant - it simply speeds up the rate of approach to equilibrium.
catalysts
state functions (thermodynamics)
equation of state
heats of formation
31. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
electromotive force (emf)/ cell
absorbs (in atomic spectra)
positive
dynamic equilibrium
32. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
...
titration
Van der Waals
kinetic molecular theory
33. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
sublimation
hydrolysis
anode rays
base - acid
34. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
temperature
Van der Waals
non-ideal
sublimation
35. Electronegativities _______ as you go down a group.
melting point
system (thermodynamics)
decreases
heat capacity
36. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
kinetic molecular theory
anode rays
left - right (Le Chatelier's principle)
third law of thermodynamics
37. A chemical reaction formed from the union of its elements.
electrolytic cells
Van der Waals
boiling point elevation
combination
38. Heat added to a system and work done by a system are considered _________ quantities.
heat capacity
isopiestic process (thermodynamics)
temperature
positive
39. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.
40. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.
increases
phase equilibrium
kinetic molecular theory
positive
41. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
2
activation energy
zero
42. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
pi bonds
crystallizes
left - right (Le Chatelier's principle)
cathode rays
43. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.
kinetic molecular theory
decomposition
electrolytic cells
titration
44. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
equivalent point
state (thermodynamics)
reversible reaction
isopiestic process (thermodynamics)
45. A catalyst lowers the ______ _____ _____ that must be overcome in order for the reaction to proceed. It merely speeds the approach to equilibrium but does not change Keq at all.
46. **Proceeding across a period from left to right - the ionization energy _______.
phase equilibrium
Van der Waals
pi bonds
increases
47. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
positive
boiling point elevation
Nernst equation
change in enthalpy
48. The change in enthalpy of an exothermic reaction is ________.
negative
electrolytic cells
Daltons law
electronegativity
49. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge
positive charge
increases
anode rays
sublimation
50. Deviations from Boyles law that occur with real gases represent _______ behavior.
anode rays
pressure
non-ideal
Van der Waals