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. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
positive charge
increases
partial


2. The vapor pressure increases with increasing _____.
upper right corner
change in enthalpy
temperature
VSEPR


3. When an electron moves from an excited state to the ground state - it _______ energy.
2
decreases
Van der Waals
emits (in atomic spectra)


4. Electronegativities ________ from left to right in a period.
adiabatic process (thermodynamics)
positive
activation energy
increases


5. 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.
left (Le Chatelier's principle)
Van der Waals
catalysts
Charles law


6. 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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7. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
kinetic molecular theory
activation energy
absorbs (in atomic spectra)


8. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
equivalent point
left (Le Chatelier's principle)
zero
boiling point


9. Rays made up of positive electrodes in basic electron charges.
electrolytic cells
equivalent point
anode rays
adiabatic process (thermodynamics)


10. The pressure exerted by each gas in a mixture is called its _____ pressure.
Nernst equation
partial
Daltons law
molar heat of sublimation


11. Deviations from Boyles law that occur with real gases represent _______ behavior.
pressure
10 degrees
non-ideal
combination


12. 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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13. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
heat capacity
Nernst equation
activation energy barrier (Le Chatelier's principle)
decreases


14. 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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15. Decreasing the concentrations of reactants shifts the equilibrium to the ______ - thus decreasing the concentration of products formed.

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16. **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.
adiabatic process (thermodynamics)
...
increases
catalysts


17. In titration - this is the point at which a particular indicator changes color.
end point
Charles law
ideal gas
catalysts


18. Liquids with strong attractive forces have ______ boiling points.
high
vapor pressure
lower left corner
temperature


19. 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.
electronegativity
boiling point
Charles law
wave mechanical model


20. 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.
total pressure (Le Chatelier's principle)
change in enthalpy
titration
Van der Waals


21. 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.
state functions (thermodynamics)
colligative property law
electrolytic reactions
negative


22. A hypothetical gas would follow Boyles law under all conditions and is called?
ideal gas
third law of thermodynamics
state (thermodynamics)
activation energy barrier (Le Chatelier's principle)


23. 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.
sublimation
pi bonds
Van der Waals
standard atmospheric pressure


24. When the electron moves from the ground state to an excited state - it ______ energy.
absorbs (in atomic spectra)
system (thermodynamics)
state functions (thermodynamics)
Avogrados law


25. 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.
positive
combined gas law
Daltons law
equivalent point


26. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
Raoult's law
kinetic molecular theory
10 degrees
Avogrados law


27. The molecules in a gas are in constant - continueous - random - and straight-line motion.
kinetic molecular theory
specific heat
Charles law
zero


28. 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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29. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
entropy
left - right (Le Chatelier's principle)
specific heat
crystallizes


30. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
kinetic molecular theory
Charles law
Boyles law
irreversible and reversible processes


31. The temperature at which a substance's solid and liquid phases are in equilibrium.
second law of thermodynamics
...
melting point
moles (Le Chatelier's principle)


32. The most active metals are found in what corner of the periodic table?
negative
lower left corner
partial
right (Le Chatelier's principle)


33. The most active nonmetals are found in what corner of the periodic table?
lower left corner
upper right corner
emits (in atomic spectra)
equilibrium


34. 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)
adiabatic process (thermodynamics)
electrolytic reactions
isothermal process (thermodynamics)


35. For a cell at concentrations and conditions other than standard - a potential can be calculated using this equation.
kinetic molecular theory
Nernst equation
left (Le Chatelier's principle)
decreases


36. 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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37. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
emits (in atomic spectra)
activation energy
high
reversible


38. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
ideal gas
Van der Waals
electrolytic reactions
activation energy barrier (Le Chatelier's principle)


39. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
Le Chatelier's principle
heat capacity
left - right (Le Chatelier's principle)
point particles


40. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
equilibrium
increases
boiling point elevation
Le Chatelier's principle


41. *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
point particles
moles (Le Chatelier's principle)


42. Electronegativities _______ as you go down a group.
limiting law
decreases
increases
lower left corner


43. 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.
equivalent point
sublimation
state functions (thermodynamics)
anode rays


44. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
state (thermodynamics)
decreases
Charles law
combined gas law


45. The freezing point is always lowered by addition of solute.
freezing point depression
positive
wave mechanical model
activation energy barrier (Le Chatelier's principle)


46. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
pressure
wave mechanical model
dynamic equilibrium
irreversible and reversible processes


47. *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.
decomposition
Van der Waals
equation of state
VSEPR


48. The degree of randomness of a system is represented by a thermodynamic quantity called? the greater the randomness - the greater the _______.
limiting law
absorbs (in atomic spectra)
entropy
reversible reaction


49. The heat change during a process carried out at a constant pressure.
equivalent point
...
right (Le Chatelier's principle)
change in enthalpy


50. **As we proceed to the right of the table - ______-forming properties decrease and _____-forming properties increase.
increases
phase equilibrium
base - acid
system (thermodynamics)