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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. 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.
combination
decomposition
Daltons law
Charles law
2. 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.
hydrolysis
kinetic molecular theory
reversible
...
3. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
electromotive force (emf)/ cell
activation energy
negative
change in enthalpy
4. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
base - acid
zero
increases
kinetic molecular theory
5. 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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6. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
base - acid
right (Le Chatelier's principle)
end point
positive
7. 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
crystallizes
system (thermodynamics)
positive
8. Electronegativities _______ as you go down a group.
base - acid
negative
point particles
decreases
9. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
first law of thermodynamics
electronegativity
irreversible and reversible processes
hybridyzation
10. 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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11. 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
melting point
positive
partial
12. A process that occurs whent eh system is maintained at constant pressure.
kinetic molecular theory
temperature
isopiestic process (thermodynamics)
catalysts
13. The most active metals are found in what corner of the periodic table?
lower left corner
increases
isothermal process (thermodynamics)
total pressure (Le Chatelier's principle)
14. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
Daltons law
left (Le Chatelier's principle)
point particles
...
15. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
left - right (Le Chatelier's principle)
state (thermodynamics)
double replacement/displacement
adiabatic process (thermodynamics)
16. When the electron moves from the ground state to an excited state - it ______ energy.
equivalent point
decomposition
absorbs (in atomic spectra)
enthalpy
17. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
single replacement/displacement
decreases
Van der Waals
third law of thermodynamics
18. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
system (thermodynamics)
point particles
isopiestic process (thermodynamics)
limiting law
19. *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.
...
equation of state
decomposition
entropy
20. The change in enthalpy of an endothermic reaction is ________.
positive
Charles law
2
heat capacity
21. The freezing point is always lowered by addition of solute.
point particles
freezing point depression
enthalpy
heat capacity
22. In an exothermic process - energy is released and ^E of reaction is ________.
pressure
hydrolysis
positive
negative
23. In an endothermic process - energy is absorbed and ^E is _______.
positive
zero
enthalpy
electrolytic cells
24. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
Valence Shell Electron Pair Repulsion (VSEPR)
wave mechanical model
increases
25. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
combined gas law
metallic
boiling point
26. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
ideal gas
boiling point
sublimation
wave mechanical model
27. A state function in which it is the heat content of a substance.
adiabatic process (thermodynamics)
right (Le Chatelier's principle)
enthalpy
heat capacity
28. Metals have electronegativities less than ____
state functions (thermodynamics)
equilibrium
Le Chatelier's principle
2
29. 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.
adiabatic process (thermodynamics)
...
electronegativity
electromotive force (emf)/ cell
30. 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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31. 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.
increases
equation of state
Daltons law
state functions (thermodynamics)
32. Liquids with strong attractive forces have ______ boiling points.
ionization energy
high
combined gas law
non-ideal
33. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
10 degrees
zero
valence
boiling point elevation
34. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
cathode rays
increases
lower left corner
state (thermodynamics)
35. When the rate of evaporation equals the rate of condensation - the system is in __________.
colligative property law
equilibrium
increases
Van der Waals
36. 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)
Charles law
crystallizes
positive charge
37. 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
isothermal process (thermodynamics)
catalysts
partial
38. Rays made up of electrons in basic electron charges.
kinetic molecular theory
cathode rays
saturated solution
bohr model
39. A hypothetical gas would follow Boyles law under all conditions and is called?
increases
catalysts
ideal gas
kinetic molecular theory
40. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
negative
decreases
ideal gas
41. This process occurs when the system is thermally isolated so that no heat enters or leaves.
combined gas law
adiabatic process (thermodynamics)
absorbs (in atomic spectra)
Charles law
42. Heat added to a system and work done by a system are considered _________ quantities.
equilibrium
positive
reversible
lower left corner
43. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
pressure
increases
kinetic molecular theory
Charles law
44. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
electrolytic reactions
irreversible and reversible processes
decreases
phase equilibrium
45. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
increases
...
bohr model
phase equilibrium
46. *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
hydrolysis
colligative property law
Boyles law
47. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
limiting law
decomposition
state (thermodynamics)
entropy
48. *The electrons found in the outermost shell are called _____ electrons. When these electrons are lost or partially lost through sharing - the oxidation state is assigned a positive value for the element. If valence electrons are gained or partially g
valence
kinetic molecular theory
kinetic molecular theory
Charles law
49. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
increases
end point
decreases
electromotive force (emf)/ cell
50. 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.
upper right corner
limiting law
Van der Waals
single replacement/displacement