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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.
change in enthalpy
titration
partial
Le Chatelier's principle
2. A state function in which it is the heat content of a substance.
heat capacity
moles (Le Chatelier's principle)
enthalpy
negative
3. 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.
positive
titration
Nernst equation
boiling point
4. 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.
enthalpy
Raoults law
negative
Daltons law
5. Rays made up of positive electrodes in basic electron charges.
activation energy
pi bonds
anode rays
catalysts
6. 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.
colligative property law
anode rays
change in enthalpy
2
7. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
second law of thermodynamics
standard atmospheric pressure
molar heat of sublimation
negative
8. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
catalysts
system (thermodynamics)
melting point
zero
9. 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).
Le Chatelier's principle
state (thermodynamics)
sublimation
negative
10. The freezing point is always lowered by addition of solute.
first law of thermodynamics
single replacement/displacement
freezing point depression
left (Le Chatelier's principle)
11. The energy required to remove an electron from an isolated atom in its ground state.
10 degrees
Daltons law
first law of thermodynamics
ionization energy
12. 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.
increasing
heats of formation
Raoults law
...
13. 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
Le Chatelier's principle
10 degrees
absorbs (in atomic spectra)
14. 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.
catalysts
Charles law
vapor pressure
titration
15. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
reversible reaction
Charles law
Nernst equation
decreases
16. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
equivalent point
base - acid
high
Raoults law
17. Metals have electronegativities less than ____
decreases
freezing point depression
upper right corner
2
18. The heat required to change 1mole of solid completely to vapor.
emits (in atomic spectra)
molar heat of sublimation
end point
equivalent point
19. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
reversible reaction
cathode rays
right (Le Chatelier's principle)
kinetic molecular theory
20. *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.
...
pressure
left - right (Le Chatelier's principle)
electrolytic cells
21. Rays made up of electrons in basic electron charges.
irreversible and reversible processes
cathode rays
reversible
boiling point
22. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
freezing point depression
activation energy
increases
23. 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.
second law of thermodynamics
isothermal process (thermodynamics)
reversible
high
24. In an endothermic process - energy is absorbed and ^E is _______.
activation energy barrier (Le Chatelier's principle)
Boyles law
positive
moles (Le Chatelier's principle)
25. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
Daltons law
catalysts
enthalpy
increasing
26. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
positive charge
Charles law
catalysts
cathode rays
27. 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).
crystallizes
second law of thermodynamics
boiling point elevation
Van der Waals
28. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
Daltons law
molar heat of sublimation
positive
29. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
base - acid
increases
left - right (Le Chatelier's principle)
Nernst equation
30. A solution in which solid solute is in equilibrium with dissolved solute.
boiling point
titration
saturated solution
Raoult's law
31. In an exothermic process - energy is released and ^E of reaction is ________.
negative
Nernst equation
second law of thermodynamics
increases
32. The most active nonmetals are found in what corner of the periodic table?
upper right corner
heat capacity
sublimation
Daltons law
33. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
activation energy
kinetic molecular theory
second law of thermodynamics
...
34. 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
irreversible and reversible processes
isopiestic process (thermodynamics)
hydrolysis
change in enthalpy
35. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
combined gas law
end point
standard atmospheric pressure
reversible reaction
36. 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
base - acid
partial
state (thermodynamics)
bohr model
37. This process occurs when the system is thermally isolated so that no heat enters or leaves.
adiabatic process (thermodynamics)
metallic
2
VSEPR
38. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
freezing point depression
equation of state
crystallizes
positive
39. 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.
40. 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.
41. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
heats of formation
reversible reaction
saturated solution
42. 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.
reversible reaction
state functions (thermodynamics)
Avogrados law
kinetic molecular theory
43. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
Avogrados law
negative
molar heat of sublimation
44. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
kinetic molecular theory
Le Chatelier's principle
entropy
45. 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.
enthalpy
Avogrados law
ionization energy
electronegativity
46. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
single replacement/displacement
increases
freezing point depression
phase equilibrium
47. *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
boiling point
ideal gas
positive
48. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
irreversible and reversible processes
hybridyzation
Avogrados law
Van der Waals
49. Electronegativities ________ from left to right in a period.
...
negative
increases
hydrolysis
50. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
crystallizes
entropy
electromotive force (emf)/ cell
isothermal process (thermodynamics)