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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. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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2. Heat added to a system and work done by a system are considered _________ quantities.
Le Chatelier's principle
increases
positive
end point
3. 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.
negative
equation of state
Charles law
vapor pressure
4. This process occurs when the system is maintained at the same temperature throughout an experiment.
isothermal process (thermodynamics)
upper right corner
right (Le Chatelier's principle)
double replacement/displacement
5. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
combined gas law
vapor pressure
single replacement/displacement
heat capacity
6. 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.
VSEPR
positive
catalysts
double replacement/displacement
7. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
combined gas law
increasing
molar heat of sublimation
8. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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9. A solution in which solid solute is in equilibrium with dissolved solute.
double replacement/displacement
crystallizes
saturated solution
change in enthalpy
10. 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.
valence
first law of thermodynamics
activation energy barrier (Le Chatelier's principle)
titration
11. 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 _____ _
zero
Charles law
limiting law
standard atmospheric pressure
12. A state function in which it is the heat content of a substance.
colligative property law
sublimation
enthalpy
...
13. 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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14. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
electrolytic cells
adiabatic process (thermodynamics)
equilibrium
15. 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
dynamic equilibrium
first law of thermodynamics
Le Chatelier's principle
irreversible and reversible processes
16. 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.
heats of formation
colligative property law
total pressure (Le Chatelier's principle)
second law of thermodynamics
17. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
Van der Waals
Avogrados law
second law of thermodynamics
Boyles law
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.
enthalpy
kinetic molecular theory
Van der Waals
hybridyzation
19. The heat change during a process carried out at a constant pressure.
change in enthalpy
Raoult's law
hydrolysis
boiling point
20. 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
kinetic molecular theory
Raoults law
second law of thermodynamics
bohr model
21. 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
positive charge
increasing
valence
boiling point elevation
22. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
bohr model
boiling point elevation
decreases
third law of thermodynamics
23. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
upper right corner
molar heat of sublimation
Nernst equation
kinetic molecular theory
24. In an endothermic process - energy is absorbed and ^E is _______.
temperature
reversible reaction
positive
zero
25. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
decomposition
third law of thermodynamics
left (Le Chatelier's principle)
crystallizes
26. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
positive charge
decreases
system (thermodynamics)
colligative property law
27. *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
combined gas law
ionization energy
Le Chatelier's principle
28. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
anode rays
reversible reaction
enthalpy
29. Electronegativities _______ as you go down a group.
Daltons law
reversible reaction
Nernst equation
decreases
30. Electronegativities ________ from left to right in a period.
upper right corner
kinetic molecular theory
increases
catalysts
31. This is due to the way positive charges of one molecule attract the negative charges of another molecule. Compounds of the solid state that are bound mainly by this type of attractive have soft crystals - are easily deformed - and vaporize easily.
2
limiting law
Van der Waals
entropy
32. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
wave mechanical model
heat capacity
dynamic equilibrium
single replacement/displacement
33. 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.
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34. In titration - this is the point at which a particular indicator changes color.
end point
partial
Boyles law
equation of state
35. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
electrolytic reactions
Van der Waals
heats of formation
boiling point elevation
36. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
dynamic equilibrium
combination
sublimation
positive
37. 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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38. The freezing point is always lowered by addition of solute.
metallic
freezing point depression
Le Chatelier's principle
electronegativity
39. The molecules in a gas are in constant - continueous - random - and straight-line motion.
positive
kinetic molecular theory
ideal gas
phase equilibrium
40. *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.
equation of state
state (thermodynamics)
metallic
positive
41. A chemical reaction formed from the union of its elements.
combination
isopiestic process (thermodynamics)
activation energy
second law of thermodynamics
42. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
increases
base - acid
adiabatic process (thermodynamics)
heats of formation
43. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
Avogrados law
electrolytic reactions
pressure
sublimation
44. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
combination
ionization energy
Boyles law
upper right corner
45. 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.
Van der Waals
Daltons law
standard atmospheric pressure
point particles
46. 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.
electronegativity
10 degrees
anode rays
wave mechanical model
47. The change in enthalpy of an endothermic reaction is ________.
positive
high
crystallizes
right (Le Chatelier's principle)
48. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
high
heat capacity
kinetic molecular theory
standard atmospheric pressure
49. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
increases
heat capacity
base - acid
electromotive force (emf)/ cell
50. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
Charles law
increasing
dynamic equilibrium
electromotive force (emf)/ cell