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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. Rays made up of electrons in basic electron charges.
lower left corner
equilibrium
cathode rays
hydrolysis
2. The pressure exerted by each gas in a mixture is called its _____ pressure.
moles (Le Chatelier's principle)
partial
hydrolysis
reversible
3. The heat required to change 1mole of solid completely to vapor.
negative
Valence Shell Electron Pair Repulsion (VSEPR)
wave mechanical model
molar heat of sublimation
4. In titration - this is the point at which a particular indicator changes color.
freezing point depression
end point
reversible
high
5. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
right (Le Chatelier's principle)
Van der Waals
Avogrados law
second law of thermodynamics
6. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
positive
crystallizes
emits (in atomic spectra)
end point
7. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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8. 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.
non-ideal
negative
kinetic molecular theory
system (thermodynamics)
9. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Le Chatelier's principle
2
system (thermodynamics)
Nernst equation
10. 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.
pressure
Boyles law
Daltons law
end point
11. In an exothermic process - energy is released and ^E of reaction is ________.
Avogrados law
pressure
negative
high
12. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
valence
double replacement/displacement
Boyles law
Charles law
13. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
Boyles law
10 degrees
Van der Waals
pi bonds
14. 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.
upper right corner
...
negative
colligative property law
15. 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.
absorbs (in atomic spectra)
system (thermodynamics)
adiabatic process (thermodynamics)
state functions (thermodynamics)
16. A solution in which solid solute is in equilibrium with dissolved solute.
decreases
saturated solution
specific heat
combined gas law
17. Liquids with strong attractive forces have ______ boiling points.
upper right corner
negative
single replacement/displacement
high
18. A process that occurs whent eh system is maintained at constant pressure.
increasing
isopiestic process (thermodynamics)
saturated solution
upper right corner
19. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
point particles
heat capacity
Le Chatelier's principle
sublimation
20. 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.
boiling point
molar heat of sublimation
combination
reversible
21. *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.
pi bonds
anode rays
end point
...
22. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
Raoult's law
change in enthalpy
zero
heats of formation
23. The most active nonmetals are found in what corner of the periodic table?
activation energy
second law of thermodynamics
left (Le Chatelier's principle)
upper right corner
24. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Charles law
Avogrados law
decreases
Boyles law
25. **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.
...
kinetic molecular theory
point particles
kinetic molecular theory
26. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
boiling point elevation
kinetic molecular theory
increasing
Raoult's law
27. When the rate of evaporation equals the rate of condensation - the system is in __________.
equilibrium
high
Van der Waals
decomposition
28. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
non-ideal
positive
electrolytic reactions
Nernst equation
29. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
kinetic molecular theory
system (thermodynamics)
positive charge
partial
30. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
entropy
catalysts
dynamic equilibrium
cathode rays
31. 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).
valence
Van der Waals
sublimation
10 degrees
32. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
vapor pressure
anode rays
reversible reaction
...
33. The molecules in a gas are in constant - continueous - random - and straight-line motion.
Valence Shell Electron Pair Repulsion (VSEPR)
kinetic molecular theory
Charles law
partial
34. The change in enthalpy of an endothermic reaction is ________.
positive
colligative property law
right (Le Chatelier's principle)
temperature
35. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
Charles law
kinetic molecular theory
change in enthalpy
Le Chatelier's principle
36. The heat change during a process carried out at a constant pressure.
cathode rays
system (thermodynamics)
change in enthalpy
dynamic equilibrium
37. 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
valence
base - acid
change in enthalpy
38. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
pressure
decreases
reversible
Nernst equation
39. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
standard atmospheric pressure
...
bohr model
entropy
40. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.
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41. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
activation energy
kinetic molecular theory
Daltons law
Le Chatelier's principle
42. 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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43. The vapor pressure increases with increasing _____.
negative
Raoult's law
temperature
kinetic molecular theory
44. 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.
first law of thermodynamics
negative
heats of formation
positive
45. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
reversible reaction
enthalpy
positive
electromotive force (emf)/ cell
46. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
isopiestic process (thermodynamics)
kinetic molecular theory
negative
combined gas law
47. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
electromotive force (emf)/ cell
dynamic equilibrium
kinetic molecular theory
third law of thermodynamics
48. 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.
increases
total pressure (Le Chatelier's principle)
state (thermodynamics)
Raoults law
49. *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.
limiting law
Le Chatelier's principle
emits (in atomic spectra)
equation of state
50. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
absorbs (in atomic spectra)
crystallizes
base - acid
hybridyzation