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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 molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
kinetic molecular theory
increases
negative
isothermal process (thermodynamics)
2. The heat change during a process carried out at a constant pressure.
pi bonds
entropy
increasing
change in enthalpy
3. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
entropy
activation energy
hybridyzation
metallic
4. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heat capacity
2
second law of thermodynamics
10 degrees
5. Liquids with strong attractive forces have ______ boiling points.
change in enthalpy
high
Le Chatelier's principle
increases
6. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
Boyles law
bohr model
kinetic molecular theory
7. Heat added to a system and work done by a system are considered _________ quantities.
combination
positive
emits (in atomic spectra)
kinetic molecular theory
8. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
phase equilibrium
2
heats of formation
sublimation
9. 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.
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10. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
third law of thermodynamics
Raoults law
equation of state
second law of thermodynamics
11. This process occurs when the system is maintained at the same temperature throughout an experiment.
equivalent point
isothermal process (thermodynamics)
titration
negative
12. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.
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13. 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.
colligative property law
valence
ideal gas
Avogrados law
14. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
Valence Shell Electron Pair Repulsion (VSEPR)
increases
electrolytic cells
15. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
electrolytic cells
first law of thermodynamics
...
decreases
16. Rays made up of positive electrodes in basic electron charges.
temperature
anode rays
end point
electromotive force (emf)/ cell
17. Cells that convert electrical energy into chemical energy.
dynamic equilibrium
Daltons law
molar heat of sublimation
electrolytic cells
18. 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
electronegativity
isothermal process (thermodynamics)
bohr model
molar heat of sublimation
19. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
Charles law
equation of state
moles (Le Chatelier's principle)
20. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
crystallizes
phase equilibrium
limiting law
state functions (thermodynamics)
21. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
emits (in atomic spectra)
kinetic molecular theory
system (thermodynamics)
22. In an exothermic process - energy is released and ^E of reaction is ________.
positive charge
base - acid
partial
negative
23. 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
electrolytic reactions
hydrolysis
kinetic molecular theory
24. This law states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in mixture.
end point
single replacement/displacement
Daltons law
lower left corner
25. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
left (Le Chatelier's principle)
Boyles law
right (Le Chatelier's principle)
26. The most active nonmetals are found in what corner of the periodic table?
...
upper right corner
system (thermodynamics)
titration
27. When the rate of evaporation equals the rate of condensation - the system is in __________.
ionization energy
heats of formation
upper right corner
equilibrium
28. A chemical reaction formed from the union of its elements.
hydrolysis
combination
cathode rays
right (Le Chatelier's principle)
29. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
decreases
kinetic molecular theory
total pressure (Le Chatelier's principle)
30. *The hypothetical ideal gas obeys exactly the mathematical statement of the ideal gas law. This statement is also called the _____ ___ ____ of an ideal gas because it relates the variables (P - V - n - T) that specify properties of the gas.
system (thermodynamics)
ionization energy
positive
equation of state
31. *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.
Raoults law
wave mechanical model
single replacement/displacement
change in enthalpy
32. The vapor pressure increases with increasing _____.
left (Le Chatelier's principle)
temperature
increases
Boyles law
33. 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.
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34. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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35. When an electron moves from an excited state to the ground state - it _______ energy.
vapor pressure
Nernst equation
emits (in atomic spectra)
limiting law
36. 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 elevation
negative
Raoults law
kinetic molecular theory
37. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.
activation energy
VSEPR
kinetic molecular theory
...
38. In titration - this is the point at which a particular indicator changes color.
second law of thermodynamics
end point
equation of state
heats of formation
39. 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 _____ _
freezing point depression
standard atmospheric pressure
kinetic molecular theory
limiting law
40. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
titration
Charles law
increases
pressure
41. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
pressure
activation energy
kinetic molecular theory
electrolytic cells
42. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
hybridyzation
wave mechanical model
electromotive force (emf)/ cell
moles (Le Chatelier's principle)
43. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
first law of thermodynamics
base - acid
moles (Le Chatelier's principle)
Boyles law
44. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.
standard atmospheric pressure
combination
state functions (thermodynamics)
Van der Waals
45. The change in enthalpy of an exothermic reaction is ________.
2
Charles law
negative
pi bonds
46. 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).
Van der Waals
absorbs (in atomic spectra)
equation of state
kinetic molecular theory
47. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
isopiestic process (thermodynamics)
kinetic molecular theory
cathode rays
heat capacity
48. When the electron moves from the ground state to an excited state - it ______ energy.
saturated solution
hydrolysis
isothermal process (thermodynamics)
absorbs (in atomic spectra)
49. The most active metals are found in what corner of the periodic table?
positive
point particles
total pressure (Le Chatelier's principle)
lower left corner
50. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
end point
positive
positive