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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. Cells that convert electrical energy into chemical energy.
heat capacity
electrolytic cells
wave mechanical model
change in enthalpy
2. 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.
Charles law
isopiestic process (thermodynamics)
kinetic molecular theory
standard atmospheric pressure
3. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
kinetic molecular theory
...
adiabatic process (thermodynamics)
increasing
4. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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5. *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.
zero
equation of state
sublimation
colligative property law
6. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
state (thermodynamics)
Valence Shell Electron Pair Repulsion (VSEPR)
single replacement/displacement
vapor pressure
7. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
entropy
Nernst equation
Avogrados law
Van der Waals
8. Rays made up of positive electrodes in basic electron charges.
anode rays
Charles law
positive charge
pressure
9. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
double replacement/displacement
total pressure (Le Chatelier's principle)
enthalpy
10. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
activation energy
standard atmospheric pressure
end point
catalysts
11. Deviations from Boyles law that occur with real gases represent _______ behavior.
absorbs (in atomic spectra)
positive
non-ideal
Van der Waals
12. 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 _____ _
2
heat capacity
Daltons law
limiting law
13. The change in enthalpy of an endothermic reaction is ________.
Valence Shell Electron Pair Repulsion (VSEPR)
positive
reversible
double replacement/displacement
14. When an electron moves from an excited state to the ground state - it _______ energy.
emits (in atomic spectra)
electronegativity
freezing point depression
ionization energy
15. 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).
decomposition
electronegativity
10 degrees
state (thermodynamics)
16. The heat required to change 1mole of solid completely to vapor.
total pressure (Le Chatelier's principle)
entropy
molar heat of sublimation
cathode rays
17. 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
molar heat of sublimation
base - acid
kinetic molecular theory
18. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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19. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
Nernst equation
heats of formation
third law of thermodynamics
positive
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
valence
melting point
state functions (thermodynamics)
bohr model
21. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
wave mechanical model
Avogrados law
hybridyzation
Van der Waals
22. Metals have electronegativities less than ____
combined gas law
decreases
Charles law
2
23. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
state functions (thermodynamics)
electromotive force (emf)/ cell
emits (in atomic spectra)
...
24. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
titration
kinetic molecular theory
Nernst equation
point particles
25. 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.
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26. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
Le Chatelier's principle
Charles law
pressure
limiting law
27. *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.
equilibrium
10 degrees
...
electromotive force (emf)/ cell
28. A hypothetical gas would follow Boyles law under all conditions and is called?
decomposition
Van der Waals
ideal gas
moles (Le Chatelier's principle)
29. Electronegativities _______ as you go down a group.
base - acid
Avogrados law
point particles
decreases
30. 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.
Nernst equation
Raoults law
phase equilibrium
state functions (thermodynamics)
31. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
decreases
increases
kinetic molecular theory
positive
32. When a system at equilibrium is disturbed by adding or removing one of hte substances - all the concentrations will change until a new equilibrium point is reached with the same value of Keq.
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33. 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
standard atmospheric pressure
emits (in atomic spectra)
dynamic equilibrium
34. A state function in which it is the heat content of a substance.
activation energy
enthalpy
saturated solution
heats of formation
35. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
boiling point
electrolytic reactions
change in enthalpy
third law of thermodynamics
36. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
Raoults law
heat capacity
ionization energy
isothermal process (thermodynamics)
37. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
specific heat
positive
electrolytic reactions
38. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
negative
molar heat of sublimation
Le Chatelier's principle
39. _____ bonds are present in molecules containing double or triple bonds.
negative
pi bonds
cathode rays
saturated solution
40. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
sublimation
Boyles law
Daltons law
phase equilibrium
41. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
VSEPR
state functions (thermodynamics)
Valence Shell Electron Pair Repulsion (VSEPR)
heats of formation
42. 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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43. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
freezing point depression
Charles law
irreversible and reversible processes
catalysts
44. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
colligative property law
total pressure (Le Chatelier's principle)
...
increases
45. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
kinetic molecular theory
phase equilibrium
increases
sublimation
46. The general shape of any molecule can be predicted from the number of bonding and non-bonding electron pairs in the valence shell of the central atom. nonbonded pairs of electrons (lone pairs) are more repellent than bonded pairs.
isothermal process (thermodynamics)
negative
VSEPR
reversible
47. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
positive
base - acid
Daltons law
zero
48. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
crystallizes
partial
activation energy
Boyles law
49. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
equivalent point
activation energy barrier (Le Chatelier's principle)
isothermal process (thermodynamics)
vapor pressure
50. Rays made up of electrons in basic electron charges.
boiling point elevation
pressure
cathode rays
negative