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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 pressure exerted by each gas in a mixture is called its _____ pressure.
partial
Van der Waals
positive
isothermal process (thermodynamics)
2. The molecules in a gas are in constant - continueous - random - and straight-line motion.
cathode rays
kinetic molecular theory
right (Le Chatelier's principle)
specific heat
3. *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.
system (thermodynamics)
equation of state
decreases
enthalpy
4. 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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5. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
Daltons law
increasing
standard atmospheric pressure
high
6. *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.
combination
Van der Waals
...
reversible reaction
7. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
positive charge
upper right corner
...
decreases
8. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
equation of state
boiling point elevation
Charles law
high
9. A process that occurs whent eh system is maintained at constant pressure.
limiting law
hydrolysis
freezing point depression
isopiestic process (thermodynamics)
10. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
kinetic molecular theory
third law of thermodynamics
end point
specific heat
11. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
phase equilibrium
bohr model
kinetic molecular theory
Daltons law
12. A solution in which solid solute is in equilibrium with dissolved solute.
partial
saturated solution
electromotive force (emf)/ cell
wave mechanical model
13. A chemical reaction formed from the union of its elements.
...
combination
boiling point elevation
standard atmospheric pressure
14. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
...
pressure
Van der Waals
Raoult's law
15. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
2
anode rays
sublimation
reversible reaction
16. 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.
increases
equivalent point
dynamic equilibrium
state (thermodynamics)
17. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
Van der Waals
10 degrees
reversible
Avogrados law
18. *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.
wave mechanical model
increases
state functions (thermodynamics)
...
19. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
change in enthalpy
Daltons law
colligative property law
...
20. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
Van der Waals
temperature
enthalpy
reversible reaction
21. The heat required to change 1mole of solid completely to vapor.
adiabatic process (thermodynamics)
molar heat of sublimation
kinetic molecular theory
equilibrium
22. 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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23. The change in enthalpy of an endothermic reaction is ________.
activation energy
left - right (Le Chatelier's principle)
kinetic molecular theory
positive
24. 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.
left - right (Le Chatelier's principle)
moles (Le Chatelier's principle)
reversible
end point
25. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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26. When an electron moves from an excited state to the ground state - it _______ energy.
vapor pressure
saturated solution
emits (in atomic spectra)
positive
27. 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.
ionization energy
electrolytic cells
adiabatic process (thermodynamics)
VSEPR
28. 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.
vapor pressure
colligative property law
Raoult's law
standard atmospheric pressure
29. 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).
increases
state (thermodynamics)
Valence Shell Electron Pair Repulsion (VSEPR)
Van der Waals
30. The change in enthalpy of an exothermic reaction is ________.
combined gas law
kinetic molecular theory
negative
total pressure (Le Chatelier's principle)
31. 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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32. 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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33. In an endothermic process - energy is absorbed and ^E is _______.
...
point particles
positive
specific heat
34. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
ideal gas
third law of thermodynamics
zero
equilibrium
35. Deviations from Boyles law that occur with real gases represent _______ behavior.
bohr model
Le Chatelier's principle
kinetic molecular theory
non-ideal
36. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
double replacement/displacement
combination
kinetic molecular theory
wave mechanical model
37. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
point particles
electronegativity
saturated solution
valence
38. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
kinetic molecular theory
activation energy
10 degrees
39. A hypothetical gas would follow Boyles law under all conditions and is called?
ideal gas
2
sublimation
Le Chatelier's principle
40. 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.
high
first law of thermodynamics
system (thermodynamics)
bohr model
41. The energy required to remove an electron from an isolated atom in its ground state.
Van der Waals
ionization energy
kinetic molecular theory
positive
42. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
dynamic equilibrium
hybridyzation
ionization energy
temperature
43. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
positive charge
reversible
double replacement/displacement
44. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
crystallizes
reversible
positive
equivalent point
45. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
10 degrees
non-ideal
metallic
reversible
46. When the electron moves from the ground state to an excited state - it ______ energy.
titration
Raoults law
absorbs (in atomic spectra)
decreases
47. Electronegativities _______ as you go down a group.
decreases
Avogrados law
point particles
first law of thermodynamics
48. Heat added to a system and work done by a system are considered _________ quantities.
positive
moles (Le Chatelier's principle)
emits (in atomic spectra)
Avogrados law
49. The temperature at which a substance's solid and liquid phases are in equilibrium.
pi bonds
saturated solution
melting point
Raoult's law
50. 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.
zero
isopiestic process (thermodynamics)
specific heat
state functions (thermodynamics)