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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 heat change during a process carried out at a constant pressure.
increases
change in enthalpy
third law of thermodynamics
Daltons law
2. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
partial
increasing
reversible
entropy
3. Heat added to a system and work done by a system are considered _________ quantities.
kinetic molecular theory
reversible reaction
heat capacity
positive
4. Metals have electronegativities less than ____
Raoults law
pressure
2
partial
5. A solution in which solid solute is in equilibrium with dissolved solute.
third law of thermodynamics
saturated solution
titration
kinetic molecular theory
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.
ionization energy
valence
...
specific heat
7. This process occurs when the system is thermally isolated so that no heat enters or leaves.
crystallizes
double replacement/displacement
adiabatic process (thermodynamics)
combined gas law
8. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
equilibrium
10 degrees
point particles
9. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
increases
specific heat
...
partial
10. **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.
heats of formation
Le Chatelier's principle
end point
...
11. Liquids with strong attractive forces have ______ boiling points.
kinetic molecular theory
high
kinetic molecular theory
crystallizes
12. In an endothermic process - energy is absorbed and ^E is _______.
melting point
equivalent point
positive
emits (in atomic spectra)
13. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
specific heat
double replacement/displacement
equilibrium
right (Le Chatelier's principle)
14. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
molar heat of sublimation
colligative property law
second law of thermodynamics
cathode rays
15. *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.
wave mechanical model
equation of state
cathode rays
pi bonds
16. The freezing point is always lowered by addition of solute.
titration
melting point
freezing point depression
point particles
17. A process that occurs whent eh system is maintained at constant pressure.
phase equilibrium
isopiestic process (thermodynamics)
isothermal process (thermodynamics)
bohr model
18. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
electrolytic reactions
increases
Boyles law
saturated solution
19. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
boiling point elevation
entropy
single replacement/displacement
20. A hypothetical gas would follow Boyles law under all conditions and is called?
increases
ideal gas
electromotive force (emf)/ cell
Van der Waals
21. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
isothermal process (thermodynamics)
positive
sublimation
vapor pressure
22. 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.
kinetic molecular theory
Le Chatelier's principle
VSEPR
decreases
23. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
point particles
base - acid
saturated solution
third law of thermodynamics
24. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
freezing point depression
kinetic molecular theory
10 degrees
25. Cells that convert electrical energy into chemical energy.
entropy
electrolytic cells
positive
combined gas law
26. 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.
kinetic molecular theory
negative
state functions (thermodynamics)
limiting law
27. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
kinetic molecular theory
heat capacity
bohr model
increases
28. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
bohr model
crystallizes
kinetic molecular theory
base - acid
29. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
phase equilibrium
negative
reversible
Van der Waals
30. 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.
positive charge
Nernst equation
equivalent point
Le Chatelier's principle
31. Electronegativities ________ from left to right in a period.
melting point
anode rays
increases
total pressure (Le Chatelier's principle)
32. The temperature at which a substance's solid and liquid phases are in equilibrium.
hybridyzation
melting point
positive charge
...
33. 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
crystallizes
vapor pressure
left - right (Le Chatelier's principle)
34. The molecules in a gas are in constant - continueous - random - and straight-line motion.
ionization energy
kinetic molecular theory
freezing point depression
pi bonds
35. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
positive
negative
upper right corner
36. 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).
left (Le Chatelier's principle)
Van der Waals
state (thermodynamics)
increases
37. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
electrolytic reactions
negative
vapor pressure
38. 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
anode rays
electronegativity
hydrolysis
39. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
temperature
equivalent point
Nernst equation
40. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
moles (Le Chatelier's principle)
anode rays
boiling point elevation
combined gas law
41. 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.
Raoults law
Daltons law
left - right (Le Chatelier's principle)
anode rays
42. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
isothermal process (thermodynamics)
Van der Waals
dynamic equilibrium
specific heat
43. 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 _____ _
limiting law
moles (Le Chatelier's principle)
emits (in atomic spectra)
kinetic molecular theory
44. 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.
45. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
equilibrium
...
standard atmospheric pressure
negative
46. The most active metals are found in what corner of the periodic table?
entropy
lower left corner
saturated solution
Raoults law
47. A chemical reaction formed from the union of its elements.
combination
titration
increases
decreases
48. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
point particles
base - acid
kinetic molecular theory
non-ideal
49. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
10 degrees
Van der Waals
...
lower left corner
50. *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.
non-ideal
combined gas law
ionization energy
wave mechanical model