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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. 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.
anode rays
state (thermodynamics)
Raoults law
electrolytic cells
2. When the electron moves from the ground state to an excited state - it ______ energy.
crystallizes
absorbs (in atomic spectra)
dynamic equilibrium
10 degrees
3. 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.
second law of thermodynamics
state (thermodynamics)
colligative property law
Le Chatelier's principle
4. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
...
kinetic molecular theory
standard atmospheric pressure
boiling point elevation
5. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
Nernst equation
entropy
increases
kinetic molecular theory
6. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
reversible
catalysts
metallic
7. 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.
entropy
vapor pressure
Valence Shell Electron Pair Repulsion (VSEPR)
negative
8. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
kinetic molecular theory
base - acid
vapor pressure
Le Chatelier's principle
9. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
melting point
single replacement/displacement
system (thermodynamics)
Nernst equation
10. The freezing point is always lowered by addition of solute.
partial
equation of state
combination
freezing point depression
11. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.
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12. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Van der Waals
Charles law
10 degrees
crystallizes
13. The pressure exerted by each gas in a mixture is called its _____ pressure.
absorbs (in atomic spectra)
partial
decreases
catalysts
14. A chemical reaction where there is an actual exchange of partners to form new compounds. ex: AgNO3 + NaCl -> AgCl + NaNO3.
heats of formation
molar heat of sublimation
double replacement/displacement
positive
15. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.
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16. This process occurs when the system is maintained at the same temperature throughout an experiment.
sublimation
2
isothermal process (thermodynamics)
heat capacity
17. 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).
emits (in atomic spectra)
combination
VSEPR
state (thermodynamics)
18. *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
Le Chatelier's principle
single replacement/displacement
wave mechanical model
19. A solution in which solid solute is in equilibrium with dissolved solute.
enthalpy
state (thermodynamics)
saturated solution
vapor pressure
20. **Proceeding across a period from left to right - the ionization energy _______.
anode rays
moles (Le Chatelier's principle)
pi bonds
increases
21. In an endothermic process - energy is absorbed and ^E is _______.
state (thermodynamics)
positive
heats of formation
phase equilibrium
22. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
VSEPR
zero
Van der Waals
enthalpy
23. The heat change during a process carried out at a constant pressure.
change in enthalpy
crystallizes
increases
hydrolysis
24. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
second law of thermodynamics
...
2
point particles
25. A state function in which it is the heat content of a substance.
negative
ideal gas
enthalpy
equation of state
26. Increasing the pressure on a system at equilibrium will cause a shift in the position of equilibrium in the direction of the fewest number of ______ of gaseous reactants or products.
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27. Cells that convert electrical energy into chemical energy.
phase equilibrium
Avogrados law
heats of formation
electrolytic cells
28. The action of salts of weak acids or bases with water to form acidic or basic solutions.
isopiestic process (thermodynamics)
hydrolysis
Valence Shell Electron Pair Repulsion (VSEPR)
anode rays
29. 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.
metallic
first law of thermodynamics
dynamic equilibrium
entropy
30. The change in enthalpy of an endothermic reaction is ________.
colligative property law
second law of thermodynamics
positive
hydrolysis
31. The energy required to remove an electron from an isolated atom in its ground state.
VSEPR
catalysts
ionization energy
boiling point elevation
32. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
wave mechanical model
reversible
decreases
second law of thermodynamics
33. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
state functions (thermodynamics)
...
boiling point
heat capacity
34. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Boyles law
...
adiabatic process (thermodynamics)
decomposition
35. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
pi bonds
...
metallic
electromotive force (emf)/ cell
36. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
negative
high
zero
decomposition
37. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
left - right (Le Chatelier's principle)
increases
Valence Shell Electron Pair Repulsion (VSEPR)
kinetic molecular theory
38. 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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39. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
activation energy
bohr model
Avogrados law
boiling point
40. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
Valence Shell Electron Pair Repulsion (VSEPR)
double replacement/displacement
dynamic equilibrium
decreases
41. 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
colligative property law
electrolytic reactions
VSEPR
42. Heat added to a system and work done by a system are considered _________ quantities.
positive
Avogrados law
isothermal process (thermodynamics)
kinetic molecular theory
43. 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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44. Rays made up of positive electrodes in basic electron charges.
double replacement/displacement
change in enthalpy
anode rays
decreases
45. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
bohr model
second law of thermodynamics
reversible reaction
boiling point
46. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
Van der Waals
boiling point elevation
single replacement/displacement
electrolytic cells
47. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
Boyles law
kinetic molecular theory
10 degrees
boiling point
48. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
sublimation
kinetic molecular theory
equilibrium
heats of formation
49. 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.
increases
positive
isothermal process (thermodynamics)
equivalent point
50. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
pressure
saturated solution
kinetic molecular theory
state (thermodynamics)