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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. 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 _____ _
positive
limiting law
2
left (Le Chatelier's principle)
2. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
single replacement/displacement
molar heat of sublimation
point particles
Boyles law
3. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
double replacement/displacement
Daltons law
total pressure (Le Chatelier's principle)
dynamic equilibrium
4. 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
Van der Waals
state (thermodynamics)
base - acid
5. The temperature at which a substance's solid and liquid phases are in equilibrium.
saturated solution
melting point
kinetic molecular theory
high
6. When an electron moves from an excited state to the ground state - it _______ energy.
right (Le Chatelier's principle)
enthalpy
emits (in atomic spectra)
positive
7. A state function in which it is the heat content of a substance.
...
hybridyzation
enthalpy
absorbs (in atomic spectra)
8. 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.
9. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
positive charge
kinetic molecular theory
increases
10. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
specific heat
...
Nernst equation
second law of thermodynamics
11. 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.
state functions (thermodynamics)
limiting law
crystallizes
reversible
12. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
Van der Waals
Raoults law
system (thermodynamics)
activation energy
13. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
positive charge
standard atmospheric pressure
valence
...
14. The molecules in a gas are in constant - continueous - random - and straight-line motion.
boiling point
Van der Waals
electromotive force (emf)/ cell
kinetic molecular theory
15. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
combined gas law
Le Chatelier's principle
negative
double replacement/displacement
16. 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.
right (Le Chatelier's principle)
electrolytic reactions
single replacement/displacement
Daltons law
17. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
negative
pressure
system (thermodynamics)
heat capacity
18. 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.
electrolytic cells
Valence Shell Electron Pair Repulsion (VSEPR)
freezing point depression
limiting law
19. 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.
kinetic molecular theory
reversible reaction
boiling point
Charles law
20. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
valence
increases
Boyles law
Charles law
21. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
metallic
positive
kinetic molecular theory
decomposition
22. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
23. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
electrolytic reactions
decreases
Le Chatelier's principle
freezing point depression
24. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
10 degrees
boiling point
electrolytic reactions
change in enthalpy
25. 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.
26. The heat change during a process carried out at a constant pressure.
kinetic molecular theory
Le Chatelier's principle
Charles law
change in enthalpy
27. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
high
10 degrees
activation energy
reversible
28. Liquids with strong attractive forces have ______ boiling points.
cathode rays
kinetic molecular theory
kinetic molecular theory
high
29. _____ bonds are present in molecules containing double or triple bonds.
irreversible and reversible processes
pi bonds
equivalent point
right (Le Chatelier's principle)
30. 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.
phase equilibrium
first law of thermodynamics
equation of state
titration
31. 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.
32. In titration - this point occurs when equal numbers of equivalents of acid and base have been reacted. The solution at this point is neutral because neither of the ions of the salt in solution undergoes hydrolysis.
equivalent point
titration
heat capacity
kinetic molecular theory
33. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
negative
negative
10 degrees
Van der Waals
34. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
10 degrees
kinetic molecular theory
standard atmospheric pressure
double replacement/displacement
35. In an exothermic process - energy is released and ^E of reaction is ________.
melting point
left (Le Chatelier's principle)
specific heat
negative
36. In an endothermic process - energy is absorbed and ^E is _______.
...
positive
sublimation
equilibrium
37. 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).
heats of formation
entropy
irreversible and reversible processes
state (thermodynamics)
38. The pressure exerted by each gas in a mixture is called its _____ pressure.
Boyles law
Nernst equation
partial
electrolytic reactions
39. A chemical reaction formed from the union of its elements.
Charles law
combination
Van der Waals
activation energy
40. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
sublimation
first law of thermodynamics
pi bonds
standard atmospheric pressure
41. The heat required to change 1mole of solid completely to vapor.
saturated solution
boiling point
reversible
molar heat of sublimation
42. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
Nernst equation
total pressure (Le Chatelier's principle)
wave mechanical model
hydrolysis
43. Electronegativities ________ from left to right in a period.
system (thermodynamics)
molar heat of sublimation
first law of thermodynamics
increases
44. 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.
Nernst equation
freezing point depression
base - acid
catalysts
45. In titration - this is the point at which a particular indicator changes color.
valence
melting point
end point
hydrolysis
46. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
boiling point elevation
saturated solution
kinetic molecular theory
vapor pressure
47. A hypothetical gas would follow Boyles law under all conditions and is called?
anode rays
ideal gas
decomposition
positive
48. Electronegativities _______ as you go down a group.
decreases
Daltons law
phase equilibrium
positive charge
49. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
decreases
phase equilibrium
Nernst equation
saturated solution
50. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
VSEPR
zero
metallic
point particles