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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. In titration - this is the point at which a particular indicator changes color.
bohr model
right (Le Chatelier's principle)
end point
Daltons law
2. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Charles law
2
Boyles law
10 degrees
3. The heat change during a process carried out at a constant pressure.
change in enthalpy
negative
end point
partial
4. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
total pressure (Le Chatelier's principle)
kinetic molecular theory
second law of thermodynamics
colligative property law
5. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
isopiestic process (thermodynamics)
ideal gas
upper right corner
single replacement/displacement
6. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
left - right (Le Chatelier's principle)
moles (Le Chatelier's principle)
titration
kinetic molecular theory
7. 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
colligative property law
pressure
sublimation
8. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
metallic
cathode rays
kinetic molecular theory
ionization energy
9. 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.
positive
non-ideal
decomposition
first law of thermodynamics
10. The action of salts of weak acids or bases with water to form acidic or basic solutions.
first law of thermodynamics
metallic
specific heat
hydrolysis
11. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
colligative property law
isopiestic process (thermodynamics)
change in enthalpy
12. 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.
increases
double replacement/displacement
reversible
equivalent point
13. The average kinetic energy of all the molecules collectively is directly proportional to the absolute temperature of the gas. The average kinetic energy of equal numbers of molecules of any gas is the same at the same temperature.
kinetic molecular theory
dynamic equilibrium
high
left - right (Le Chatelier's principle)
14. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
change in enthalpy
positive
sublimation
Nernst equation
15. 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.
16. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
second law of thermodynamics
point particles
freezing point depression
base - acid
17. The temperature at which a substance's solid and liquid phases are in equilibrium.
increases
melting point
double replacement/displacement
equilibrium
18. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
19. The heat required to change 1mole of solid completely to vapor.
isothermal process (thermodynamics)
metallic
left - right (Le Chatelier's principle)
molar heat of sublimation
20. 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.
21. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
colligative property law
combination
partial
dynamic equilibrium
22. In an exothermic process - energy is released and ^E of reaction is ________.
wave mechanical model
negative
increases
change in enthalpy
23. *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
combined gas law
entropy
valence
high
24. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
catalysts
Valence Shell Electron Pair Repulsion (VSEPR)
sublimation
increasing
25. This process occurs when the system is maintained at the same temperature throughout an experiment.
electromotive force (emf)/ cell
isothermal process (thermodynamics)
equivalent point
colligative property law
26. In an endothermic process - energy is absorbed and ^E is _______.
standard atmospheric pressure
positive
combination
second law of thermodynamics
27. The ________ of an element is a number that measerures the relative strength in which the atoms of the element attract valence electrons in a chemical bond - on a scale of 0-4.
Boyles law
state functions (thermodynamics)
electronegativity
Le Chatelier's principle
28. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
valence
moles (Le Chatelier's principle)
specific heat
sublimation
29. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
ionization energy
change in enthalpy
positive
30. 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.
state functions (thermodynamics)
saturated solution
adiabatic process (thermodynamics)
ionization energy
31. A hypothetical gas would follow Boyles law under all conditions and is called?
kinetic molecular theory
Charles law
Nernst equation
ideal gas
32. 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 _____ _
kinetic molecular theory
10 degrees
Charles law
limiting law
33. Electronegativities _______ as you go down a group.
decreases
left - right (Le Chatelier's principle)
Daltons law
Le Chatelier's principle
34. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
hydrolysis
crystallizes
positive
heats of formation
35. Metals have electronegativities less than ____
zero
2
adiabatic process (thermodynamics)
...
36. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
increases
Van der Waals
lower left corner
change in enthalpy
37. The most active nonmetals are found in what corner of the periodic table?
first law of thermodynamics
pressure
positive charge
upper right corner
38. _____ bonds are present in molecules containing double or triple bonds.
pi bonds
high
Valence Shell Electron Pair Repulsion (VSEPR)
Boyles law
39. The vapor pressure increases with increasing _____.
first law of thermodynamics
temperature
pressure
absorbs (in atomic spectra)
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.
Boyles law
...
kinetic molecular theory
decomposition
41. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
valence
positive
electromotive force (emf)/ cell
electrolytic reactions
42. A solution in which solid solute is in equilibrium with dissolved solute.
activation energy barrier (Le Chatelier's principle)
10 degrees
saturated solution
irreversible and reversible processes
43. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
moles (Le Chatelier's principle)
second law of thermodynamics
kinetic molecular theory
negative
44. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
system (thermodynamics)
wave mechanical model
kinetic molecular theory
heat capacity
45. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
...
change in enthalpy
Boyles law
46. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
Van der Waals
ideal gas
crystallizes
increases
47. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
saturated solution
emits (in atomic spectra)
pressure
zero
48. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
ideal gas
isopiestic process (thermodynamics)
state functions (thermodynamics)
49. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
equilibrium
boiling point
combination
lower left corner
50. When the rate of evaporation equals the rate of condensation - the system is in __________.
partial
standard atmospheric pressure
equilibrium
...