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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. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
kinetic molecular theory
partial
equivalent point
electrolytic reactions
2. In titration - this is the point at which a particular indicator changes color.
end point
non-ideal
irreversible and reversible processes
entropy
3. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
anode rays
heat capacity
Van der Waals
boiling point
4. 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.
Charles law
specific heat
equivalent point
combined gas law
5. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
increasing
phase equilibrium
upper right corner
third law of thermodynamics
6. 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.
colligative property law
kinetic molecular theory
upper right corner
change in enthalpy
7. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
Van der Waals
non-ideal
vapor pressure
isothermal process (thermodynamics)
8. In a closed system - when the rates of evaporation and condensation are equal - the system is in ____ ______.
total pressure (Le Chatelier's principle)
temperature
phase equilibrium
Boyles law
9. 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.
dynamic equilibrium
Charles law
VSEPR
sublimation
10. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
2
kinetic molecular theory
left (Le Chatelier's principle)
specific heat
11. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
non-ideal
moles (Le Chatelier's principle)
activation energy
cathode rays
12. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
colligative property law
activation energy
entropy
state functions (thermodynamics)
13. The vapor pressure increases with increasing _____.
second law of thermodynamics
non-ideal
temperature
dynamic equilibrium
14. A chemical reaction formed from the union of its elements.
combination
catalysts
system (thermodynamics)
Charles law
15. This process occurs when the system is thermally isolated so that no heat enters or leaves.
activation energy
reversible
adiabatic process (thermodynamics)
valence
16. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
limiting law
Valence Shell Electron Pair Repulsion (VSEPR)
...
isothermal process (thermodynamics)
17. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
end point
single replacement/displacement
dynamic equilibrium
increases
18. 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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19. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
Charles law
partial
activation energy
combined gas law
20. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
freezing point depression
positive charge
system (thermodynamics)
partial
21. Electronegativities _______ as you go down a group.
lower left corner
reversible
decreases
Van der Waals
22. The pressure exerted by each gas in a mixture is called its _____ pressure.
double replacement/displacement
first law of thermodynamics
increases
partial
23. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
metallic
Raoult's law
kinetic molecular theory
activation energy
24. The energy required to remove an electron from an isolated atom in its ground state.
upper right corner
absorbs (in atomic spectra)
ionization energy
anode rays
25. The action of salts of weak acids or bases with water to form acidic or basic solutions.
emits (in atomic spectra)
hydrolysis
state functions (thermodynamics)
non-ideal
26. The most active nonmetals are found in what corner of the periodic table?
Raoults law
limiting law
upper right corner
hydrolysis
27. 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 _____ _
hydrolysis
limiting law
single replacement/displacement
melting point
28. 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.
reversible
positive
phase equilibrium
first law of thermodynamics
29. 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
state functions (thermodynamics)
boiling point elevation
Raoults law
30. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
double replacement/displacement
increases
dynamic equilibrium
hydrolysis
31. 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.
partial
ionization energy
melting point
Daltons law
32. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
Van der Waals
Avogrados law
Charles law
molar heat of sublimation
33. 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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34. This process occurs when the system is maintained at the same temperature throughout an experiment.
Raoult's law
10 degrees
Daltons law
isothermal process (thermodynamics)
35. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
Van der Waals
zero
standard atmospheric pressure
anode rays
36. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
positive
reversible reaction
positive charge
37. 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.
wave mechanical model
kinetic molecular theory
right (Le Chatelier's principle)
absorbs (in atomic spectra)
38. In an exothermic process - energy is released and ^E of reaction is ________.
negative
Le Chatelier's principle
electromotive force (emf)/ cell
decomposition
39. For a ________ reaction - the energy liberated in the exothermic reaction equals the energy absorbed in the endothermic reaction.
negative
kinetic molecular theory
positive charge
reversible reaction
40. 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.
hydrolysis
heats of formation
standard atmospheric pressure
titration
41. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
Le Chatelier's principle
colligative property law
VSEPR
42. 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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43. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
Le Chatelier's principle
decomposition
standard atmospheric pressure
increases
44. The pressure of a gas is the result of collisions between the gas molecules and the walls of the container.
system (thermodynamics)
Le Chatelier's principle
kinetic molecular theory
electrolytic cells
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. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
system (thermodynamics)
left - right (Le Chatelier's principle)
positive charge
double replacement/displacement
47. When the rate of evaporation equals the rate of condensation - the system is in __________.
electronegativity
equilibrium
Raoult's law
crystallizes
48. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
temperature
Le Chatelier's principle
decomposition
non-ideal
49. **Five factors that affect reaction rates: 1. The nature of the reactants and products. 2. The surface area exposed. 3. The concentrations. 4. The temperature. 5. The catalyst.
reversible
negative
...
kinetic molecular theory
50. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
boiling point
upper right corner
Van der Waals
increases