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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. This process occurs when the system is maintained at the same temperature throughout an experiment.
increases
isothermal process (thermodynamics)
Charles law
isopiestic process (thermodynamics)
2. In an exothermic process - energy is released and ^E of reaction is ________.
negative
vapor pressure
partial
irreversible and reversible processes
3. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
Daltons law
molar heat of sublimation
positive
heats of formation
4. 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.
5. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
single replacement/displacement
melting point
increases
electrolytic cells
6. Rays made up of positive electrodes in basic electron charges.
molar heat of sublimation
positive
zero
anode rays
7. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
second law of thermodynamics
increases
specific heat
isopiestic process (thermodynamics)
8. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
decomposition
entropy
2
total pressure (Le Chatelier's principle)
9. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
pressure
kinetic molecular theory
electrolytic reactions
specific heat
10. The heat required to change 1mole of solid completely to vapor.
negative
left - right (Le Chatelier's principle)
molar heat of sublimation
2
11. 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 elevation
temperature
2
sublimation
12. This process occurs when the system is thermally isolated so that no heat enters or leaves.
positive charge
absorbs (in atomic spectra)
adiabatic process (thermodynamics)
Nernst equation
13. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
combination
electromotive force (emf)/ cell
...
enthalpy
14. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
boiling point elevation
vapor pressure
hydrolysis
15. 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
melting point
equilibrium
positive charge
colligative property law
16. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.
titration
combination
partial
...
17. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
valence
...
...
18. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
sublimation
lower left corner
double replacement/displacement
Van der Waals
19. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
vapor pressure
heats of formation
base - acid
dynamic equilibrium
20. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
reversible reaction
vapor pressure
Van der Waals
crystallizes
21. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
increasing
kinetic molecular theory
high
third law of thermodynamics
22. 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
single replacement/displacement
molar heat of sublimation
electronegativity
23. A state function in which it is the heat content of a substance.
boiling point
Charles law
enthalpy
change in enthalpy
24. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
25. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heat capacity
titration
molar heat of sublimation
Le Chatelier's principle
26. A hypothetical gas would follow Boyles law under all conditions and is called?
...
reversible
ideal gas
boiling point elevation
27. The ______ of the system is some particular set of conditions of pressure - temperature - number of moles of each component - and their physical form (ex: gas - liquid - solid or crystalline form).
2
equivalent point
positive charge
state (thermodynamics)
28. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
end point
Van der Waals
Charles law
kinetic molecular theory
29. 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.
30. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
boiling point
ideal gas
metallic
base - acid
31. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
hydrolysis
lower left corner
dynamic equilibrium
combined gas law
32. 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.
activation energy barrier (Le Chatelier's principle)
Raoults law
specific heat
total pressure (Le Chatelier's principle)
33. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
molar heat of sublimation
isothermal process (thermodynamics)
Raoult's law
electromotive force (emf)/ cell
34. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
hydrolysis
Avogrados law
ionization energy
35. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
2
increasing
decreases
isothermal process (thermodynamics)
36. In an endothermic process - energy is absorbed and ^E is _______.
positive
boiling point
standard atmospheric pressure
...
37. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
reversible
change in enthalpy
boiling point
point particles
38. The temperature at which a substance's solid and liquid phases are in equilibrium.
Charles law
...
state (thermodynamics)
melting point
39. *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.
Van der Waals
...
kinetic molecular theory
negative
40. 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.
molar heat of sublimation
increases
ionization energy
colligative property law
41. *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
boiling point elevation
valence
zero
third law of thermodynamics
42. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
electrolytic reactions
Raoult's law
moles (Le Chatelier's principle)
hybridyzation
43. The freezing point is always lowered by addition of solute.
combination
freezing point depression
saturated solution
emits (in atomic spectra)
44. 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.
catalysts
state functions (thermodynamics)
wave mechanical model
third law of thermodynamics
45. When the rate of evaporation equals the rate of condensation - the system is in __________.
...
equilibrium
2
moles (Le Chatelier's principle)
46. Liquids with strong attractive forces have ______ boiling points.
high
increasing
Charles law
irreversible and reversible processes
47. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
...
pressure
irreversible and reversible processes
negative
48. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
double replacement/displacement
negative
freezing point depression
standard atmospheric pressure
49. A valence theory that permits the geometric arrangement of atoms - or groups of atoms - about some central atom to be determined solely by considering the repulsions between the electron pairs present in the valence shell of the central atom.
heats of formation
adiabatic process (thermodynamics)
decomposition
Valence Shell Electron Pair Repulsion (VSEPR)
50. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
positive charge
increases
emits (in atomic spectra)
system (thermodynamics)