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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. **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.
equilibrium
...
boiling point
melting point
2. 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.
3. A hypothetical gas would follow Boyles law under all conditions and is called?
enthalpy
electrolytic cells
end point
ideal gas
4. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
system (thermodynamics)
entropy
third law of thermodynamics
increases
5. 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.
absorbs (in atomic spectra)
...
equivalent point
standard atmospheric pressure
6. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
phase equilibrium
increases
cathode rays
boiling point
7. 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.
8. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
non-ideal
irreversible and reversible processes
Charles law
combined gas law
9. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
vapor pressure
partial
kinetic molecular theory
positive charge
10. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Charles law
equilibrium
equivalent point
kinetic molecular theory
11. The vapor pressure increases with increasing _____.
adiabatic process (thermodynamics)
lower left corner
isopiestic process (thermodynamics)
temperature
12. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
boiling point
increases
Raoult's law
emits (in atomic spectra)
13. 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.
...
crystallizes
Raoults law
Van der Waals
14. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
ideal gas
limiting law
heats of formation
decreases
15. 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.
positive
Daltons law
ionization energy
point particles
16. 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.
17. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
18. When the electron moves from the ground state to an excited state - it ______ energy.
saturated solution
combination
increases
absorbs (in atomic spectra)
19. The change in enthalpy of an exothermic reaction is ________.
molar heat of sublimation
2
negative
absorbs (in atomic spectra)
20. Rays made up of electrons in basic electron charges.
left - right (Le Chatelier's principle)
ionization energy
reversible reaction
cathode rays
21. 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.
increases
ionization energy
base - acid
VSEPR
22. *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.
Le Chatelier's principle
increases
right (Le Chatelier's principle)
wave mechanical model
23. Deviations from Boyles law that occur with real gases represent _______ behavior.
2
phase equilibrium
anode rays
non-ideal
24. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
Charles law
electrolytic cells
total pressure (Le Chatelier's principle)
25. Heat added to a system and work done by a system are considered _________ quantities.
equivalent point
cathode rays
positive
...
26. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
freezing point depression
state functions (thermodynamics)
positive
boiling point elevation
27. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
adiabatic process (thermodynamics)
decreases
crystallizes
kinetic molecular theory
28. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
kinetic molecular theory
state functions (thermodynamics)
saturated solution
29. 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
electrolytic cells
bohr model
colligative property law
state functions (thermodynamics)
30. 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.
end point
kinetic molecular theory
standard atmospheric pressure
hydrolysis
31. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
positive charge
Raoult's law
hybridyzation
vapor pressure
32. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
kinetic molecular theory
pi bonds
base - acid
colligative property law
33. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
boiling point elevation
positive
Boyles law
electrolytic reactions
34. A process that occurs whent eh system is maintained at constant pressure.
ideal gas
kinetic molecular theory
VSEPR
isopiestic process (thermodynamics)
35. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
wave mechanical model
Avogrados law
decreases
non-ideal
36. In an exothermic process - energy is released and ^E of reaction is ________.
lower left corner
negative
total pressure (Le Chatelier's principle)
partial
37. 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
partial
colligative property law
hybridyzation
38. Rays made up of positive electrodes in basic electron charges.
anode rays
absorbs (in atomic spectra)
Raoults law
Le Chatelier's principle
39. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
Charles law
kinetic molecular theory
specific heat
Le Chatelier's principle
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.
upper right corner
titration
decomposition
10 degrees
41. The freezing point is always lowered by addition of solute.
ionization energy
increases
Charles law
freezing point depression
42. 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 _____ _
kinetic molecular theory
Boyles law
limiting law
zero
43. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
Raoult's law
dynamic equilibrium
heat capacity
activation energy barrier (Le Chatelier's principle)
44. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
ionization energy
...
metallic
45. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
specific heat
adiabatic process (thermodynamics)
Daltons law
sublimation
46. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
heat capacity
partial
second law of thermodynamics
47. When an electron moves from an excited state to the ground state - it _______ energy.
kinetic molecular theory
...
emits (in atomic spectra)
metallic
48. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
catalysts
phase equilibrium
combination
increases
49. 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.
adiabatic process (thermodynamics)
Nernst equation
dynamic equilibrium
state functions (thermodynamics)
50. Metals have electronegativities less than ____
colligative property law
Le Chatelier's principle
positive
2