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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. 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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2. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
increasing
reversible reaction
entropy
temperature
3. When the electron moves from the ground state to an excited state - it ______ energy.
emits (in atomic spectra)
absorbs (in atomic spectra)
second law of thermodynamics
Valence Shell Electron Pair Repulsion (VSEPR)
4. The heat required to change 1mole of solid completely to vapor.
bohr model
isothermal process (thermodynamics)
equation of state
molar heat of sublimation
5. 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.
crystallizes
Le Chatelier's principle
catalysts
temperature
6. Rays made up of electrons in basic electron charges.
cathode rays
boiling point
reversible
negative
7. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
hydrolysis
kinetic molecular theory
entropy
heats of formation
8. 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.
equivalent point
Avogrados law
heats of formation
reversible
9. The action of salts of weak acids or bases with water to form acidic or basic solutions.
vapor pressure
standard atmospheric pressure
kinetic molecular theory
hydrolysis
10. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
kinetic molecular theory
wave mechanical model
single replacement/displacement
hybridyzation
11. 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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12. *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.
positive
electrolytic cells
...
dynamic equilibrium
13. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
increasing
titration
Boyles law
...
14. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
decreases
activation energy
standard atmospheric pressure
decreases
15. Heat added to a system and work done by a system are considered _________ quantities.
positive
adiabatic process (thermodynamics)
end point
decomposition
16. 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
state functions (thermodynamics)
irreversible and reversible processes
positive charge
17. 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).
Van der Waals
pi bonds
increases
molar heat of sublimation
18. Cells that convert electrical energy into chemical energy.
enthalpy
Raoults law
equivalent point
electrolytic cells
19. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
saturated solution
left - right (Le Chatelier's principle)
...
phase equilibrium
20. Liquids with strong attractive forces have ______ boiling points.
equation of state
phase equilibrium
high
decomposition
21. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
heat capacity
2
zero
positive
22. The most active metals are found in what corner of the periodic table?
single replacement/displacement
Daltons law
emits (in atomic spectra)
lower left corner
23. The most active nonmetals are found in what corner of the periodic table?
kinetic molecular theory
equilibrium
upper right corner
decomposition
24. The change in enthalpy of an endothermic reaction is ________.
equivalent point
positive
activation energy barrier (Le Chatelier's principle)
combination
25. A solution in which solid solute is in equilibrium with dissolved solute.
boiling point
wave mechanical model
saturated solution
crystallizes
26. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
increases
positive charge
lower left corner
equilibrium
27. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
Avogrados law
enthalpy
Le Chatelier's principle
heat capacity
28. 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.
right (Le Chatelier's principle)
Daltons law
colligative property law
Nernst equation
29. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge
positive charge
enthalpy
dynamic equilibrium
positive
30. The heat change during a process carried out at a constant pressure.
equation of state
boiling point elevation
change in enthalpy
standard atmospheric pressure
31. 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
boiling point elevation
decomposition
combined gas law
32. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
Nernst equation
Van der Waals
equivalent point
isopiestic process (thermodynamics)
33. *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.
specific heat
Raoults law
Charles law
wave mechanical model
34. Rays made up of positive electrodes in basic electron charges.
total pressure (Le Chatelier's principle)
phase equilibrium
upper right corner
anode rays
35. Electronegativities ________ from left to right in a period.
increases
absorbs (in atomic spectra)
positive
2
36. _____ bonds are present in molecules containing double or triple bonds.
isopiestic process (thermodynamics)
pi bonds
reversible
moles (Le Chatelier's principle)
37. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
saturated solution
boiling point
crystallizes
Van der Waals
38. In an exothermic process - energy is released and ^E of reaction is ________.
negative
lower left corner
activation energy
catalysts
39. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
saturated solution
second law of thermodynamics
Charles law
limiting law
40. Electronegativities _______ as you go down a group.
catalysts
decreases
equation of state
activation energy barrier (Le Chatelier's principle)
41. 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 _____ _
end point
limiting law
upper right corner
Valence Shell Electron Pair Repulsion (VSEPR)
42. The change in enthalpy of an exothermic reaction is ________.
negative
hybridyzation
freezing point depression
irreversible and reversible processes
43. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
point particles
Charles law
state functions (thermodynamics)
double replacement/displacement
44. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
VSEPR
zero
vapor pressure
45. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
equilibrium
partial
titration
46. A state function in which it is the heat content of a substance.
partial
freezing point depression
positive
enthalpy
47. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
ionization energy
kinetic molecular theory
limiting law
double replacement/displacement
48. 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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49. This process occurs when the system is thermally isolated so that no heat enters or leaves.
Van der Waals
VSEPR
adiabatic process (thermodynamics)
third law of thermodynamics
50. *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
electrolytic cells
valence
left - right (Le Chatelier's principle)
entropy