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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 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.
Nernst equation
kinetic molecular theory
dynamic equilibrium
lower left corner
2. *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.
electronegativity
anode rays
valence
wave mechanical model
3. Deviations from Boyles law that occur with real gases represent _______ behavior.
system (thermodynamics)
non-ideal
temperature
hybridyzation
4. 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).
system (thermodynamics)
temperature
increases
Van der Waals
5. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
Van der Waals
entropy
Valence Shell Electron Pair Repulsion (VSEPR)
activation energy
6. _____ bonds are present in molecules containing double or triple bonds.
kinetic molecular theory
adiabatic process (thermodynamics)
pi bonds
sublimation
7. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
total pressure (Le Chatelier's principle)
upper right corner
base - acid
equilibrium
8. The freezing point is always lowered by addition of solute.
Valence Shell Electron Pair Repulsion (VSEPR)
freezing point depression
equivalent point
anode rays
9. *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.
sublimation
Charles law
equation of state
combination
10. 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).
state (thermodynamics)
positive
first law of thermodynamics
kinetic molecular theory
11. Rays made up of electrons in basic electron charges.
10 degrees
isothermal process (thermodynamics)
electromotive force (emf)/ cell
cathode rays
12. Metals have electronegativities less than ____
emits (in atomic spectra)
activation energy
system (thermodynamics)
2
13. The heat change during a process carried out at a constant pressure.
change in enthalpy
zero
non-ideal
electromotive force (emf)/ cell
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.
electromotive force (emf)/ cell
Raoults law
change in enthalpy
moles (Le Chatelier's principle)
15. **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.
Valence Shell Electron Pair Repulsion (VSEPR)
...
freezing point depression
ionization energy
16. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
metallic
temperature
negative
decomposition
17. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
isothermal process (thermodynamics)
cathode rays
electrolytic cells
18. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
...
kinetic molecular theory
first law of thermodynamics
crystallizes
19. Cells that convert electrical energy into chemical energy.
partial
lower left corner
electrolytic cells
base - acid
20. An increase in temperature causes the position of equilibrium of an exothermic reaction to be shifted to the _____ - while that of and endothermic reactions is shifted to the _______.
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21. 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.
Charles law
negative
Daltons law
system (thermodynamics)
22. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
boiling point elevation
Avogrados law
anode rays
kinetic molecular theory
23. 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.
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24. The molecules in a gas are in constant - continueous - random - and straight-line motion.
lower left corner
hybridyzation
kinetic molecular theory
third law of thermodynamics
25. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
Le Chatelier's principle
Van der Waals
kinetic molecular theory
26. In titration - this is the point at which a particular indicator changes color.
Charles law
hydrolysis
Charles law
end point
27. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
lower left corner
kinetic molecular theory
base - acid
entropy
28. 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
positive
Charles law
combination
29. The energy required to remove an electron from an isolated atom in its ground state.
increases
wave mechanical model
ionization energy
base - acid
30. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
activation energy barrier (Le Chatelier's principle)
Le Chatelier's principle
pi bonds
31. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
Van der Waals
electromotive force (emf)/ cell
kinetic molecular theory
boiling point
32. When the rate of evaporation equals the rate of condensation - the system is in __________.
Boyles law
equilibrium
heats of formation
electrolytic cells
33. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
Raoults law
pressure
heats of formation
boiling point
34. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
valence
combined gas law
titration
10 degrees
35. A state function in which it is the heat content of a substance.
Charles law
enthalpy
left - right (Le Chatelier's principle)
system (thermodynamics)
36. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
combined gas law
Charles law
activation energy
colligative property law
37. The pressure exerted by each gas in a mixture is called its _____ pressure.
zero
wave mechanical model
metallic
partial
38. Heat added to a system and work done by a system are considered _________ quantities.
pi bonds
left (Le Chatelier's principle)
positive
Van der Waals
39. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
vapor pressure
titration
VSEPR
anode rays
40. The action of salts of weak acids or bases with water to form acidic or basic solutions.
ionization energy
hydrolysis
...
metallic
41. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Boyles law
zero
catalysts
2
42. The most active metals are found in what corner of the periodic table?
right (Le Chatelier's principle)
decreases
lower left corner
titration
43. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
Nernst equation
kinetic molecular theory
specific heat
partial
44. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
titration
phase equilibrium
electrolytic cells
Charles law
45. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
Van der Waals
electromotive force (emf)/ cell
positive charge
kinetic molecular theory
46. If an inert gas is introduced into a reaction vessel containing other gases at equilibrium - it will cause an increase in the ______ _____ within the container - but the increase will not affect the position of equilibrium.
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47. A process that occurs whent eh system is maintained at constant pressure.
third law of thermodynamics
sublimation
isopiestic process (thermodynamics)
ideal gas
48. 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
pressure
state functions (thermodynamics)
equilibrium
49. When the electron moves from the ground state to an excited state - it ______ energy.
valence
positive
absorbs (in atomic spectra)
increases
50. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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