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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 pressure exerted by the gas molecules when they are in equilibrium with the liquid.
equation of state
state (thermodynamics)
vapor pressure
reversible reaction
2. A state function in which it is the heat content of a substance.
anode rays
base - acid
enthalpy
pressure
3. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.
4. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
emits (in atomic spectra)
change in enthalpy
third law of thermodynamics
activation energy barrier (Le Chatelier's principle)
5. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
metallic
first law of thermodynamics
total pressure (Le Chatelier's principle)
6. This process occurs when the system is thermally isolated so that no heat enters or leaves.
ideal gas
isopiestic process (thermodynamics)
positive
adiabatic process (thermodynamics)
7. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
negative
sublimation
Nernst equation
8. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
Van der Waals
increasing
activation energy
electronegativity
9. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
specific heat
emits (in atomic spectra)
activation energy
10. The most active nonmetals are found in what corner of the periodic table?
left - right (Le Chatelier's principle)
...
upper right corner
titration
11. Rays made up of positive electrodes in basic electron charges.
activation energy
first law of thermodynamics
specific heat
anode rays
12. A hypothetical gas would follow Boyles law under all conditions and is called?
third law of thermodynamics
ideal gas
equilibrium
standard atmospheric pressure
13. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.
third law of thermodynamics
Charles law
left - right (Le Chatelier's principle)
adiabatic process (thermodynamics)
14. Real gases act in a less than ideal way - especially under conditions of increased pressure and/or decreased temperture. Real gas behavior approaches that of ideal gases as the gas pressure becomes very low. The ideal gas is thus considered a _____ _
heats of formation
limiting law
Van der Waals
vapor pressure
15. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.
16. In an exothermic process - energy is released and ^E of reaction is ________.
saturated solution
negative
Charles law
specific heat
17. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
Charles law
end point
adiabatic process (thermodynamics)
18. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.
electronegativity
base - acid
single replacement/displacement
second law of thermodynamics
19. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
...
standard atmospheric pressure
adiabatic process (thermodynamics)
20. The heat required to change 1mole of solid completely to vapor.
Nernst equation
electromotive force (emf)/ cell
VSEPR
molar heat of sublimation
21. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
freezing point depression
dynamic equilibrium
Avogrados law
ionization energy
22. 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.
reversible reaction
decomposition
catalysts
entropy
23. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
colligative property law
state functions (thermodynamics)
point particles
second law of thermodynamics
24. A theory of the hydrogen atom stating that the electron can exist in only certain stable energy levels and that when the electronic state of the atom changes - it must absorb or emit exactly that amound of energy equal to the difference betweent he f
...
positive charge
bohr model
decreases
25. In an endothermic process - energy is absorbed and ^E is _______.
electromotive force (emf)/ cell
positive
electrolytic cells
saturated solution
26. 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.
non-ideal
titration
equivalent point
temperature
27. 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.
titration
Daltons law
decreases
entropy
28. 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.
Boyles law
state functions (thermodynamics)
wave mechanical model
colligative property law
29. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
increases
total pressure (Le Chatelier's principle)
negative
heats of formation
30. The energy required to remove an electron from an isolated atom in its ground state.
positive
ionization energy
kinetic molecular theory
increases
31. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
vapor pressure
crystallizes
Van der Waals
irreversible and reversible processes
32. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
entropy
heat capacity
isothermal process (thermodynamics)
33. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
temperature
Boyles law
total pressure (Le Chatelier's principle)
kinetic molecular theory
34. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
standard atmospheric pressure
kinetic molecular theory
metallic
sublimation
35. 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.
metallic
Raoult's law
high
Raoults law
36. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
electrolytic cells
melting point
state functions (thermodynamics)
boiling point elevation
37. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
end point
10 degrees
left - right (Le Chatelier's principle)
reversible
38. *Each wave function corresponds to a certain electron energy and describes a region about the nucleus (orbital) where an electron having that energy may be found.
equation of state
electronegativity
molar heat of sublimation
wave mechanical model
39. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heats of formation
equation of state
heat capacity
change in enthalpy
40. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
41. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
left (Le Chatelier's principle)
high
first law of thermodynamics
base - acid
42. _____ bonds are present in molecules containing double or triple bonds.
equivalent point
vapor pressure
pi bonds
boiling point elevation
43. 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).
electrolytic reactions
Van der Waals
...
state functions (thermodynamics)
44. The maximum work derived from any change will be obtained only if the process is carried out in a reversible manner. All real - spontaneous changes are therefore not reversible - and the work that can be derived from an irreversible change is alway l
Raoults law
activation energy barrier (Le Chatelier's principle)
enthalpy
irreversible and reversible processes
45. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
base - acid
kinetic molecular theory
ideal gas
point particles
46. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
negative
Charles law
entropy
double replacement/displacement
47. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
third law of thermodynamics
lower left corner
...
48. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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
zero
positive charge
colligative property law
temperature
50. Electronegativities ________ from left to right in a period.
Charles law
absorbs (in atomic spectra)
increases
Avogrados law