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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. If this law was strictly obeyed - gases would not condense when they are cooled. This means that gases behave in an ideal fashion only at relatively high temperatures and low pressures.
positive charge
Charles law
molar heat of sublimation
saturated solution
2. 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.
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3. This process occurs when the system is thermally isolated so that no heat enters or leaves.
Valence Shell Electron Pair Repulsion (VSEPR)
adiabatic process (thermodynamics)
third law of thermodynamics
...
4. When the rate of evaporation equals the rate of condensation - the system is in __________.
isothermal process (thermodynamics)
equilibrium
Boyles law
single replacement/displacement
5. 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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6. A chemical reaction formed from the union of its elements.
electrolytic reactions
combination
activation energy barrier (Le Chatelier's principle)
positive
7. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
positive
upper right corner
catalysts
combined gas law
8. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
decreases
valence
activation energy barrier (Le Chatelier's principle)
9. Cells that convert electrical energy into chemical energy.
hybridyzation
electrolytic cells
metallic
point particles
10. The temperature at which a substance's solid and liquid phases are in equilibrium.
kinetic molecular theory
total pressure (Le Chatelier's principle)
reversible
melting point
11. 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.
Van der Waals
kinetic molecular theory
electrolytic cells
Raoult's law
12. A solution in which solid solute is in equilibrium with dissolved solute.
left - right (Le Chatelier's principle)
saturated solution
VSEPR
increasing
13. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
boiling point elevation
decreases
Charles law
14. Electronegativities _______ as you go down a group.
isopiestic process (thermodynamics)
decreases
kinetic molecular theory
2
15. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
catalysts
activation energy barrier (Le Chatelier's principle)
ionization energy
16. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
decreases
boiling point elevation
electromotive force (emf)/ cell
point particles
17. 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
bohr model
Boyles law
hydrolysis
positive
18. The vapor pressure increases with increasing _____.
hydrolysis
temperature
absorbs (in atomic spectra)
total pressure (Le Chatelier's principle)
19. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
absorbs (in atomic spectra)
pressure
second law of thermodynamics
20. 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
boiling point elevation
double replacement/displacement
21. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
reversible reaction
heat capacity
ionization energy
isopiestic process (thermodynamics)
22. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
Van der Waals
increases
change in enthalpy
kinetic molecular theory
23. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
activation energy barrier (Le Chatelier's principle)
VSEPR
colligative property law
24. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
wave mechanical model
activation energy
sublimation
Van der Waals
25. Electronegativities ________ from left to right in a period.
kinetic molecular theory
increases
upper right corner
kinetic molecular theory
26. In an endothermic process - energy is absorbed and ^E is _______.
reversible
decreases
positive
positive charge
27. 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.
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28. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
right (Le Chatelier's principle)
melting point
temperature
electromotive force (emf)/ cell
29. In titration - this is the point at which a particular indicator changes color.
left (Le Chatelier's principle)
entropy
double replacement/displacement
end point
30. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
hydrolysis
activation energy
absorbs (in atomic spectra)
10 degrees
31. 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.
Raoults law
equivalent point
reversible
positive charge
32. The heat change during a process carried out at a constant pressure.
change in enthalpy
hybridyzation
2
crystallizes
33. *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.
electromotive force (emf)/ cell
partial
entropy
equation of state
34. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
negative
hybridyzation
2
kinetic molecular theory
35. 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.
kinetic molecular theory
boiling point elevation
positive
reversible
36. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
positive charge
catalysts
lower left corner
crystallizes
37. Metals have electronegativities less than ____
2
double replacement/displacement
hydrolysis
lower left corner
38. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
total pressure (Le Chatelier's principle)
zero
limiting law
39. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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40. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
phase equilibrium
left (Le Chatelier's principle)
electrolytic reactions
kinetic molecular theory
41. 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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42. A hypothetical gas would follow Boyles law under all conditions and is called?
ideal gas
molar heat of sublimation
Nernst equation
Van der Waals
43. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
isopiestic process (thermodynamics)
increases
Boyles law
single replacement/displacement
44. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
state (thermodynamics)
electrolytic reactions
zero
increases
45. The freezing point is always lowered by addition of solute.
freezing point depression
non-ideal
first law of thermodynamics
electronegativity
46. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
end point
Charles law
heat capacity
decreases
47. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
boiling point
left - right (Le Chatelier's principle)
non-ideal
entropy
48. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
boiling point
vapor pressure
limiting law
dynamic equilibrium
49. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
colligative property law
melting point
reversible reaction
50. 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.
entropy
colligative property law
upper right corner
third law of thermodynamics