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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 _____ 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.
metallic
molar heat of sublimation
decreases
catalysts
2. Rays made up of electrons in basic electron charges.
increases
activation energy
Nernst equation
cathode rays
3. Electronegativities _______ as you go down a group.
catalysts
decreases
specific heat
metallic
4. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
pressure
...
entropy
5. When the rate of evaporation equals the rate of condensation - the system is in __________.
positive
increases
equilibrium
base - acid
6. *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.
increases
third law of thermodynamics
decreases
wave mechanical model
7. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
specific heat
increases
negative
lower left corner
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.
reversible
vapor pressure
decomposition
2
9. 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.
kinetic molecular theory
left - right (Le Chatelier's principle)
Charles law
electromotive force (emf)/ cell
10. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
activation energy
reversible reaction
metallic
crystallizes
11. Liquids with strong attractive forces have ______ boiling points.
decomposition
Van der Waals
negative
high
12. The vapor pressure increases with increasing _____.
activation energy
...
system (thermodynamics)
temperature
13. 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.
14. A law stating that the vapor pressure of a solution at a particular temperature is equal to teh mole fraction of the solvent in the liquid phase multiplied by the vapor pressure of the pure solvent at the same temperature.
decreases
Raoults law
positive
cathode rays
15. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
Van der Waals
...
decreases
pressure
16. 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
reversible reaction
vapor pressure
irreversible and reversible processes
point particles
17. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
metallic
titration
Van der Waals
Boyles law
18. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
positive
anode rays
...
19. The heat change during a process carried out at a constant pressure.
electronegativity
...
change in enthalpy
second law of thermodynamics
20. The change in enthalpy of an exothermic reaction is ________.
Daltons law
negative
reversible
increases
21. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
22. 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
Charles law
...
bohr model
equation of state
23. 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.
equivalent point
Raoults law
system (thermodynamics)
entropy
24. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
increases
lower left corner
reversible
25. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
colligative property law
heat capacity
increases
decomposition
26. This process occurs when the system is thermally isolated so that no heat enters or leaves.
combination
change in enthalpy
adiabatic process (thermodynamics)
boiling point elevation
27. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
reversible reaction
single replacement/displacement
bohr model
irreversible and reversible processes
28. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
molar heat of sublimation
Le Chatelier's principle
ionization energy
29. *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
phase equilibrium
temperature
valence
decomposition
30. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
heat capacity
Nernst equation
boiling point
wave mechanical model
31. 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.
first law of thermodynamics
absorbs (in atomic spectra)
reversible
...
32. The molecules in a gas are in constant - continueous - random - and straight-line motion.
partial
equilibrium
Valence Shell Electron Pair Repulsion (VSEPR)
kinetic molecular theory
33. A chemical reaction formed from the union of its elements.
entropy
positive
reversible
combination
34. 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.
end point
Daltons law
kinetic molecular theory
Van der Waals
35. 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.
ideal gas
state functions (thermodynamics)
increases
valence
36. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
titration
kinetic molecular theory
single replacement/displacement
electromotive force (emf)/ cell
37. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
38. The heat required to change 1mole of solid completely to vapor.
metallic
reversible reaction
left - right (Le Chatelier's principle)
molar heat of sublimation
39. A state function in which it is the heat content of a substance.
cathode rays
enthalpy
...
2
40. **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.
...
Van der Waals
non-ideal
Raoults law
41. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
second law of thermodynamics
isothermal process (thermodynamics)
positive
specific heat
42. _____ bonds are present in molecules containing double or triple bonds.
pi bonds
kinetic molecular theory
Van der Waals
Nernst equation
43. *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.
single replacement/displacement
...
hydrolysis
10 degrees
44. 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.
base - acid
catalysts
Van der Waals
Avogrados law
45. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
irreversible and reversible processes
electrolytic reactions
positive
melting point
46. Cells that convert electrical energy into chemical energy.
metallic
electrolytic cells
third law of thermodynamics
second law of thermodynamics
47. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
heat capacity
point particles
freezing point depression
boiling point elevation
48. In titration - this is the point at which a particular indicator changes color.
end point
saturated solution
Van der Waals
combination
49. A process that occurs whent eh system is maintained at constant pressure.
equivalent point
Van der Waals
isopiestic process (thermodynamics)
Van der Waals
50. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
Charles law
double replacement/displacement
decreases
catalysts