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Test your basic knowledge |
CLEP Chemistry 1
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Subjects
:
clep
,
science
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
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.
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. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
non-ideal
state functions (thermodynamics)
phase equilibrium
Raoult's law
2. Deviations from Boyles law that occur with real gases represent _______ behavior.
2
non-ideal
high
heats of formation
3. **Proceeding across a period from left to right - the ionization energy _______.
equilibrium
phase equilibrium
system (thermodynamics)
increases
4. The change in enthalpy of an exothermic reaction is ________.
negative
valence
enthalpy
first law of thermodynamics
5. When the rate of evaporation equals the rate of condensation - the system is in __________.
kinetic molecular theory
equilibrium
Raoult's law
right (Le Chatelier's principle)
6. Electronegativities ________ from left to right in a period.
total pressure (Le Chatelier's principle)
increases
zero
moles (Le Chatelier's principle)
7. 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)
colligative property law
bohr model
wave mechanical model
8. The temperature at which a substance's solid and liquid phases are in equilibrium.
titration
melting point
...
wave mechanical model
9. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
end point
specific heat
negative
kinetic molecular theory
10. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
Raoults law
negative
combined gas law
kinetic molecular theory
11. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
negative
dynamic equilibrium
kinetic molecular theory
activation energy barrier (Le Chatelier's principle)
12. The process of determining the amount of a solution of known concentration that is required to react completely with a certain amount of a sample that is being analyzed.
saturated solution
titration
combination
equilibrium
13. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
pressure
...
phase equilibrium
Nernst equation
14. 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
high
Nernst equation
15. This process occurs when the system is thermally isolated so that no heat enters or leaves.
absorbs (in atomic spectra)
adiabatic process (thermodynamics)
combined gas law
10 degrees
16. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
adiabatic process (thermodynamics)
second law of thermodynamics
activation energy
right (Le Chatelier's principle)
17. 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
irreversible and reversible processes
kinetic molecular theory
isopiestic process (thermodynamics)
18. In an exothermic process - energy is released and ^E of reaction is ________.
Van der Waals
absorbs (in atomic spectra)
negative
freezing point depression
19. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
metallic
reversible reaction
second law of thermodynamics
left - right (Le Chatelier's principle)
20. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
...
increasing
decomposition
positive
21. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
hybridyzation
activation energy
hydrolysis
total pressure (Le Chatelier's principle)
22. 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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23. *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.
Van der Waals
right (Le Chatelier's principle)
enthalpy
...
24. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
positive
decreases
Van der Waals
reversible reaction
25. The energy required to remove an electron from an isolated atom in its ground state.
Le Chatelier's principle
ionization energy
boiling point
temperature
26. The vapor pressure increases with increasing _____.
colligative property law
increases
temperature
positive charge
27. Heat added to a system and work done by a system are considered _________ quantities.
positive
Charles law
electrolytic reactions
melting point
28. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
dynamic equilibrium
decreases
crystallizes
enthalpy
29. The most active nonmetals are found in what corner of the periodic table?
upper right corner
third law of thermodynamics
activation energy
Daltons law
30. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
...
kinetic molecular theory
positive
pressure
31. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
increases
negative
positive
electrolytic reactions
32. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
third law of thermodynamics
kinetic molecular theory
boiling point elevation
Le Chatelier's principle
33. 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.
system (thermodynamics)
positive
increases
Charles law
34. 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.
adiabatic process (thermodynamics)
reversible reaction
titration
equivalent point
35. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
upper right corner
...
kinetic molecular theory
vapor pressure
36. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
left - right (Le Chatelier's principle)
vapor pressure
activation energy
Nernst equation
37. 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.
Le Chatelier's principle
Charles law
kinetic molecular theory
Raoults law
38. 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.
boiling point
Avogrados law
Van der Waals
base - acid
39. The heat change during a process carried out at a constant pressure.
wave mechanical model
change in enthalpy
base - acid
electronegativity
40. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
zero
Van der Waals
upper right corner
equilibrium
41. 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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42. 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.
melting point
adiabatic process (thermodynamics)
electromotive force (emf)/ cell
Valence Shell Electron Pair Repulsion (VSEPR)
43. In titration - this is the point at which a particular indicator changes color.
irreversible and reversible processes
end point
titration
left - right (Le Chatelier's principle)
44. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
heats of formation
metallic
cathode rays
isothermal process (thermodynamics)
45. 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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46. 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.
saturated solution
Raoult's law
state functions (thermodynamics)
combination
47. Rays made up of positive electrodes in basic electron charges.
isothermal process (thermodynamics)
anode rays
first law of thermodynamics
total pressure (Le Chatelier's principle)
48. The action of salts of weak acids or bases with water to form acidic or basic solutions.
hydrolysis
end point
10 degrees
activation energy barrier (Le Chatelier's principle)
49. The molecules in a gas are in constant - continueous - random - and straight-line motion.
saturated solution
Valence Shell Electron Pair Repulsion (VSEPR)
kinetic molecular theory
first law of thermodynamics
50. A hypothetical gas would follow Boyles law under all conditions and is called?
absorbs (in atomic spectra)
ideal gas
equilibrium
Van der Waals
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