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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 particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
zero
reversible reaction
Van der Waals
system (thermodynamics)
2. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
zero
catalysts
double replacement/displacement
standard atmospheric pressure
3. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
equilibrium
boiling point
...
4. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
enthalpy
electrolytic reactions
catalysts
heat capacity
5. The action of salts of weak acids or bases with water to form acidic or basic solutions.
phase equilibrium
state functions (thermodynamics)
hydrolysis
adiabatic process (thermodynamics)
6. In an exothermic process - energy is released and ^E of reaction is ________.
negative
total pressure (Le Chatelier's principle)
crystallizes
Avogrados law
7. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
saturated solution
2
kinetic molecular theory
valence
8. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
electromotive force (emf)/ cell
entropy
left (Le Chatelier's principle)
9. *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.
...
end point
kinetic molecular theory
wave mechanical model
10. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
Avogrados law
boiling point
electromotive force (emf)/ cell
10 degrees
11. _____ bonds are present in molecules containing double or triple bonds.
pi bonds
electromotive force (emf)/ cell
dynamic equilibrium
right (Le Chatelier's principle)
12. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
left (Le Chatelier's principle)
standard atmospheric pressure
decreases
VSEPR
13. Heat added to a system and work done by a system are considered _________ quantities.
adiabatic process (thermodynamics)
Charles law
left (Le Chatelier's principle)
positive
14. 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.
pressure
kinetic molecular theory
Van der Waals
Nernst equation
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).
activation energy
Van der Waals
Charles law
decomposition
16. The change in enthalpy of an exothermic reaction is ________.
upper right corner
positive
negative
vapor pressure
17. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
decreases
heats of formation
cathode rays
pressure
18. Rays made up of positive electrodes in basic electron charges.
anode rays
end point
10 degrees
absorbs (in atomic spectra)
19. 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.
melting point
Van der Waals
saturated solution
VSEPR
20. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
increases
kinetic molecular theory
phase equilibrium
left (Le Chatelier's principle)
21. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
...
absorbs (in atomic spectra)
hybridyzation
dynamic equilibrium
22. 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
freezing point depression
left - right (Le Chatelier's principle)
increases
irreversible and reversible processes
23. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
kinetic molecular theory
state functions (thermodynamics)
heats of formation
24. Metals have electronegativities less than ____
heats of formation
melting point
2
negative
25. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
decomposition
isopiestic process (thermodynamics)
pressure
specific heat
26. Deviations from Boyles law that occur with real gases represent _______ behavior.
combined gas law
positive
non-ideal
change in enthalpy
27. 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.
Daltons law
high
reversible reaction
electrolytic reactions
28. 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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29. A process that occurs whent eh system is maintained at constant pressure.
base - acid
isopiestic process (thermodynamics)
lower left corner
Nernst equation
30. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
kinetic molecular theory
electrolytic cells
melting point
31. 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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32. The heat required to change 1mole of solid completely to vapor.
molar heat of sublimation
kinetic molecular theory
catalysts
Charles law
33. The most active nonmetals are found in what corner of the periodic table?
decomposition
upper right corner
dynamic equilibrium
absorbs (in atomic spectra)
34. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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35. The temperature at which a substance's solid and liquid phases are in equilibrium.
decreases
electronegativity
melting point
heats of formation
36. 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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37. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).
kinetic molecular theory
Van der Waals
equilibrium
state (thermodynamics)
38. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
decreases
Raoults law
temperature
combined gas law
39. Rays made up of electrons in basic electron charges.
isothermal process (thermodynamics)
lower left corner
cathode rays
negative
40. 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.
isothermal process (thermodynamics)
single replacement/displacement
titration
temperature
41. 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.
specific heat
partial
Valence Shell Electron Pair Repulsion (VSEPR)
first law of thermodynamics
42. When the rate of evaporation equals the rate of condensation - the system is in __________.
adiabatic process (thermodynamics)
change in enthalpy
combination
equilibrium
43. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
enthalpy
boiling point elevation
point particles
44. 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.
Raoult's law
Charles law
upper right corner
change in enthalpy
45. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
kinetic molecular theory
partial
crystallizes
increases
46. A solution in which solid solute is in equilibrium with dissolved solute.
equation of state
kinetic molecular theory
saturated solution
right (Le Chatelier's principle)
47. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
metallic
...
third law of thermodynamics
vapor pressure
48. 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.
bohr model
Valence Shell Electron Pair Repulsion (VSEPR)
Charles law
equivalent point
49. Cells that convert electrical energy into chemical energy.
catalysts
state functions (thermodynamics)
electrolytic cells
metallic
50. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
decomposition
heat capacity
reversible reaction
cathode rays