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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. 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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2. In an exothermic process - energy is released and ^E of reaction is ________.
zero
boiling point elevation
negative
electrolytic cells
3. A hypothetical gas would follow Boyles law under all conditions and is called?
electronegativity
ideal gas
combination
Charles law
4. The most active metals are found in what corner of the periodic table?
cathode rays
kinetic molecular theory
lower left corner
end point
5. 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.
Charles law
pi bonds
phase equilibrium
vapor pressure
6. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
equilibrium
state (thermodynamics)
system (thermodynamics)
Avogrados law
7. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
electronegativity
electrolytic cells
zero
phase equilibrium
8. The energy required to remove an electron from an isolated atom in its ground state.
kinetic molecular theory
double replacement/displacement
negative
ionization energy
9. 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 _____ _
reversible
limiting law
melting point
kinetic molecular theory
10. The heat required to change 1mole of solid completely to vapor.
isopiestic process (thermodynamics)
catalysts
...
molar heat of sublimation
11. In titration - this is the point at which a particular indicator changes color.
sublimation
end point
increases
positive
12. **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.
kinetic molecular theory
...
positive
increases
13. A process that occurs whent eh system is maintained at constant pressure.
boiling point
Van der Waals
isopiestic process (thermodynamics)
catalysts
14. The pressure exerted by each gas in a mixture is called its _____ pressure.
positive
electronegativity
third law of thermodynamics
partial
15. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
...
molar heat of sublimation
moles (Le Chatelier's principle)
electronegativity
16. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
single replacement/displacement
heat capacity
kinetic molecular theory
heats of formation
17. The molecules in a gas are in constant - continueous - random - and straight-line motion.
increases
pressure
kinetic molecular theory
positive
18. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
equilibrium
negative
hybridyzation
kinetic molecular theory
19. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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20. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
irreversible and reversible processes
Le Chatelier's principle
enthalpy
metallic
21. 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.
hybridyzation
colligative property law
electronegativity
sublimation
22. The most active nonmetals are found in what corner of the periodic table?
upper right corner
decomposition
isothermal process (thermodynamics)
increases
23. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
wave mechanical model
vapor pressure
entropy
zero
24. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
...
2
hybridyzation
kinetic molecular theory
25. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
left - right (Le Chatelier's principle)
Le Chatelier's principle
single replacement/displacement
kinetic molecular theory
26. This process occurs when the system is maintained at the same temperature throughout an experiment.
positive
crystallizes
isothermal process (thermodynamics)
second law of thermodynamics
27. The change in enthalpy of an endothermic reaction is ________.
catalysts
change in enthalpy
positive
colligative property law
28. The vapor pressure increases with increasing _____.
heat capacity
anode rays
temperature
Van der Waals
29. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
equilibrium
10 degrees
decreases
emits (in atomic spectra)
30. 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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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. 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.
positive
electrolytic reactions
reversible
specific heat
33. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
adiabatic process (thermodynamics)
boiling point elevation
zero
Daltons law
34. A chemical reaction formed from the union of its elements.
standard atmospheric pressure
dynamic equilibrium
combination
total pressure (Le Chatelier's principle)
35. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g
specific heat
valence
Raoult's law
dynamic equilibrium
36. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
total pressure (Le Chatelier's principle)
hydrolysis
kinetic molecular theory
dynamic equilibrium
37. In an endothermic process - energy is absorbed and ^E is _______.
combination
positive
Avogrados law
Le Chatelier's principle
38. This process occurs when the system is thermally isolated so that no heat enters or leaves.
electronegativity
kinetic molecular theory
double replacement/displacement
adiabatic process (thermodynamics)
39. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
enthalpy
bohr model
negative
Van der Waals
40. *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.
...
reversible reaction
point particles
end point
41. The action of salts of weak acids or bases with water to form acidic or basic solutions.
partial
hydrolysis
valence
combined gas law
42. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
sublimation
partial
electrolytic reactions
kinetic molecular theory
43. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
activation energy
hybridyzation
absorbs (in atomic spectra)
reversible reaction
44. Deviations from Boyles law that occur with real gases represent _______ behavior.
Van der Waals
non-ideal
electromotive force (emf)/ cell
upper right corner
45. Rays made up of electrons in basic electron charges.
state functions (thermodynamics)
ionization energy
cathode rays
enthalpy
46. *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.
Boyles law
equation of state
Valence Shell Electron Pair Repulsion (VSEPR)
heats of formation
47. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
left - right (Le Chatelier's principle)
hybridyzation
decreases
lower left corner
48. 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
hydrolysis
2
double replacement/displacement
irreversible and reversible processes
49. 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.
upper right corner
equivalent point
Daltons law
negative
50. 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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