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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. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
electrolytic reactions
kinetic molecular theory
state functions (thermodynamics)
combination
2. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
positive
decreases
electrolytic cells
3. The change in enthalpy of an exothermic reaction is ________.
high
negative
boiling point
base - acid
4. The most active metals are found in what corner of the periodic table?
negative
Avogrados law
increasing
lower left corner
5. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
kinetic molecular theory
base - acid
phase equilibrium
activation energy barrier (Le Chatelier's principle)
6. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
right (Le Chatelier's principle)
zero
limiting law
reversible reaction
7. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
boiling point elevation
system (thermodynamics)
absorbs (in atomic spectra)
specific heat
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.
double replacement/displacement
bohr model
kinetic molecular theory
colligative property law
9. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
state (thermodynamics)
wave mechanical model
activation energy
combined gas law
10. 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.
kinetic molecular theory
Van der Waals
electrolytic cells
hydrolysis
11. The freezing point is always lowered by addition of solute.
freezing point depression
double replacement/displacement
change in enthalpy
total pressure (Le Chatelier's principle)
12. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
first law of thermodynamics
2
Charles law
third law of thermodynamics
13. Rays made up of positive electrodes in basic electron charges.
Van der Waals
anode rays
sublimation
melting point
14. 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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15. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
equivalent point
phase equilibrium
bohr model
Nernst equation
16. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
vapor pressure
zero
single replacement/displacement
point particles
17. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
activation energy
colligative property law
positive charge
18. The change in enthalpy of an endothermic reaction is ________.
valence
colligative property law
equivalent point
positive
19. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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20. 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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21. A solution in which solid solute is in equilibrium with dissolved solute.
crystallizes
saturated solution
VSEPR
heats of formation
22. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
10 degrees
cathode rays
positive
Nernst equation
23. A process that occurs whent eh system is maintained at constant pressure.
phase equilibrium
isopiestic process (thermodynamics)
saturated solution
kinetic molecular theory
24. Cells that convert electrical energy into chemical energy.
decreases
upper right corner
moles (Le Chatelier's principle)
electrolytic cells
25. 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
emits (in atomic spectra)
bohr model
vapor pressure
...
26. When an electron moves from an excited state to the ground state - it _______ energy.
sublimation
emits (in atomic spectra)
change in enthalpy
Avogrados law
27. 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 _______.
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28. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
single replacement/displacement
kinetic molecular theory
ionization energy
Daltons law
29. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
high
ideal gas
...
electrolytic reactions
30. 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.
upper right corner
Charles law
kinetic molecular theory
10 degrees
31. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
metallic
2
pressure
kinetic molecular theory
32. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
electronegativity
equation of state
heat capacity
isopiestic process (thermodynamics)
33. 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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34. 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.
moles (Le Chatelier's principle)
state functions (thermodynamics)
kinetic molecular theory
reversible
35. The molecules in a gas are in constant - continueous - random - and straight-line motion.
end point
dynamic equilibrium
...
kinetic molecular theory
36. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
Valence Shell Electron Pair Repulsion (VSEPR)
Le Chatelier's principle
increases
37. The vapor pressure increases with increasing _____.
temperature
partial
increases
Van der Waals
38. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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39. 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
Nernst equation
irreversible and reversible processes
decomposition
catalysts
40. When the electron moves from the ground state to an excited state - it ______ energy.
emits (in atomic spectra)
absorbs (in atomic spectra)
...
decreases
41. When the rate of evaporation equals the rate of condensation - the system is in __________.
Boyles law
limiting law
equilibrium
molar heat of sublimation
42. 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.
increasing
electronegativity
phase equilibrium
reversible reaction
43. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
zero
vapor pressure
cathode rays
heats of formation
44. Heat added to a system and work done by a system are considered _________ quantities.
activation energy
positive
Le Chatelier's principle
phase equilibrium
45. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
Boyles law
dynamic equilibrium
equation of state
ionization energy
46. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
entropy
Avogrados law
bohr model
kinetic molecular theory
47. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
kinetic molecular theory
positive
melting point
electromotive force (emf)/ cell
48. 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.
heat capacity
increasing
temperature
catalysts
49. 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.
anode rays
absorbs (in atomic spectra)
electronegativity
kinetic molecular theory
50. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
adiabatic process (thermodynamics)
...
temperature
cathode rays