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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 degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
reversible reaction
equivalent point
electronegativity
entropy
2. Rays made up of electrons in basic electron charges.
vapor pressure
cathode rays
10 degrees
ideal gas
3. When the electron moves from the ground state to an excited state - it ______ energy.
Van der Waals
reversible
negative
absorbs (in atomic spectra)
4. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.
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5. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
decreases
equilibrium
wave mechanical model
6. The action of salts of weak acids or bases with water to form acidic or basic solutions.
electrolytic cells
VSEPR
hydrolysis
Le Chatelier's principle
7. 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.
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8. 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
negative
left (Le Chatelier's principle)
Van der Waals
9. A principle stating that when a system at equilibrium is disturbed by the application of a stress (change in temperature - pressure - or concentration) it reacts to minimize the stress and attain a new equilibrium position.
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10. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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11. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
wave mechanical model
upper right corner
standard atmospheric pressure
freezing point depression
12. 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.
equivalent point
absorbs (in atomic spectra)
pressure
hybridyzation
13. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
equilibrium
ionization energy
positive charge
Boyles law
14. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
standard atmospheric pressure
system (thermodynamics)
freezing point depression
Van der Waals
15. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
upper right corner
metallic
first law of thermodynamics
increasing
16. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
state functions (thermodynamics)
decomposition
titration
Valence Shell Electron Pair Repulsion (VSEPR)
17. A process that occurs whent eh system is maintained at constant pressure.
combined gas law
negative
catalysts
isopiestic process (thermodynamics)
18. The change in enthalpy of an exothermic reaction is ________.
isothermal process (thermodynamics)
increases
decreases
negative
19. **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.
2
...
electrolytic reactions
kinetic molecular theory
20. 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.
reversible reaction
ionization energy
decreases
state functions (thermodynamics)
21. The vapor pressure increases with increasing _____.
saturated solution
temperature
Van der Waals
high
22. In an exothermic process - energy is released and ^E of reaction is ________.
Raoult's law
activation energy
activation energy barrier (Le Chatelier's principle)
negative
23. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
right (Le Chatelier's principle)
isopiestic process (thermodynamics)
moles (Le Chatelier's principle)
24. The freezing point is always lowered by addition of solute.
Le Chatelier's principle
melting point
positive
freezing point depression
25. The pressure exerted by each gas in a mixture is called its _____ pressure.
moles (Le Chatelier's principle)
increases
crystallizes
partial
26. 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.
reversible
melting point
Raoults law
total pressure (Le Chatelier's principle)
27. 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.
entropy
anode rays
combination
electronegativity
28. 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.
change in enthalpy
first law of thermodynamics
dynamic equilibrium
Raoults law
29. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.
Valence Shell Electron Pair Repulsion (VSEPR)
single replacement/displacement
enthalpy
2
30. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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31. Deviations from Boyles law that occur with real gases represent _______ behavior.
non-ideal
Charles law
reversible
Le Chatelier's principle
32. 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.
increases
Avogrados law
Charles law
vapor pressure
33. The heat required to change 1mole of solid completely to vapor.
increasing
heat capacity
standard atmospheric pressure
molar heat of sublimation
34. 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.
single replacement/displacement
temperature
kinetic molecular theory
isothermal process (thermodynamics)
35. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
Avogrados law
negative
positive
36. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
valence
decreases
hybridyzation
metallic
37. 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).
kinetic molecular theory
Van der Waals
phase equilibrium
positive
38. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
bohr model
...
boiling point elevation
limiting law
39. Cells that convert electrical energy into chemical energy.
second law of thermodynamics
change in enthalpy
electrolytic cells
third law of thermodynamics
40. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
non-ideal
Boyles law
reversible reaction
41. 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.
moles (Le Chatelier's principle)
Van der Waals
catalysts
adiabatic process (thermodynamics)
42. A solution in which solid solute is in equilibrium with dissolved solute.
saturated solution
crystallizes
increases
negative
43. 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.
left - right (Le Chatelier's principle)
Daltons law
irreversible and reversible processes
equilibrium
44. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
right (Le Chatelier's principle)
cathode rays
decomposition
reversible reaction
45. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
second law of thermodynamics
decreases
Boyles law
...
46. A chemical reaction formed from the union of its elements.
combination
Charles law
end point
catalysts
47. 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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48. 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 _____ _
limiting law
anode rays
hybridyzation
temperature
49. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
electromotive force (emf)/ cell
combined gas law
point particles
negative
50. This process occurs when the system is thermally isolated so that no heat enters or leaves.
Avogrados law
positive
ionization energy
adiabatic process (thermodynamics)