Instructions:

• Answer 50 questions in 15 minutes.
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• Match each statement with the correct term.
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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. 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.
isopiestic process (thermodynamics)
catalysts
saturated solution
Le Chatelier's principle


2. Deviations from Boyles law that occur with real gases represent _______ behavior.
combined gas law
end point
vapor pressure
non-ideal


3. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
negative
point particles
state (thermodynamics)
equilibrium


4. A solution in which solid solute is in equilibrium with dissolved solute.
non-ideal
hydrolysis
wave mechanical model
saturated solution


5. The temperature at which the pressure of vapor escaping from the liquid equals atmospheric pressure.
Van der Waals
increasing
boiling point
high


6. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
decreases
absorbs (in atomic spectra)
boiling point
increases


7. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
kinetic molecular theory
lower left corner
standard atmospheric pressure
vapor pressure


8. 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
high
electromotive force (emf)/ cell
state functions (thermodynamics)


9. In an exothermic process - energy is released and ^E of reaction is ________.
Charles law
end point
negative
10 degrees


10. 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.
Van der Waals
hybridyzation
base - acid
Valence Shell Electron Pair Repulsion (VSEPR)


11. The vapor pressure increases with increasing _____.
equivalent point
sublimation
temperature
decreases


12. *The Concentration usually _____ the chemical reaction rate with increasing concentrations of the reactants.
upper right corner
lower left corner
second law of thermodynamics
increases


13. The action of salts of weak acids or bases with water to form acidic or basic solutions.
total pressure (Le Chatelier's principle)
hydrolysis
positive charge
ionization energy


14. Because of the low intermolecular forces - the melting points are low and evaporation takes place so easily that it may occur at room temperature.
kinetic molecular theory
first law of thermodynamics
positive
Van der Waals


15. Electronegativities ________ from left to right in a period.
negative
upper right corner
specific heat
increases


16. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
Avogrados law
hybridyzation
state (thermodynamics)
state functions (thermodynamics)


17. Rays made up of positive electrodes in basic electron charges.
Valence Shell Electron Pair Repulsion (VSEPR)
decreases
anode rays
Le Chatelier's principle


18. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
colligative property law
kinetic molecular theory
single replacement/displacement
right (Le Chatelier's principle)


19. This process occurs when the system is maintained at the same temperature throughout an experiment.
decreases
isothermal process (thermodynamics)
saturated solution
freezing point depression


20. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
change in enthalpy
increases
Raoults law
third law of thermodynamics


21. When an electron moves from an excited state to the ground state - it _______ energy.
electrolytic reactions
second law of thermodynamics
left (Le Chatelier's principle)
emits (in atomic spectra)


22. The heat change during a process carried out at a constant pressure.
change in enthalpy
Raoult's law
moles (Le Chatelier's principle)
equilibrium


23. The change in enthalpy of an endothermic reaction is ________.
increases
positive
equation of state
non-ideal


24. In a closed system - when opposing changes are taking place at equal rates - the system is said to be in _____ _______.
left - right (Le Chatelier's principle)
dynamic equilibrium
Boyles law
decomposition


25. 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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26. Metals have electronegativities less than ____
2
kinetic molecular theory
non-ideal
state functions (thermodynamics)


27. The most active nonmetals are found in what corner of the periodic table?
moles (Le Chatelier's principle)
upper right corner
hydrolysis
Charles law


28. For a solution in which a nonvolatile solute is dissolved in a solvent - the vapor pressure is due only to the vapor of the solvent above the solution. This vapor pressure is given by _______ law.

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29. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
electromotive force (emf)/ cell
first law of thermodynamics
10 degrees
irreversible and reversible processes


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.
reversible
end point
Raoults law
anode rays


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

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32. Rays made up of electrons in basic electron charges.
negative
reversible
cathode rays
upper right corner


33. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
boiling point elevation
adiabatic process (thermodynamics)
moles (Le Chatelier's principle)
equation of state


34. This process occurs when the system is thermally isolated so that no heat enters or leaves.
specific heat
boiling point
adiabatic process (thermodynamics)
upper right corner


35. The heat required to change 1mole of solid completely to vapor.
lower left corner
kinetic molecular theory
molar heat of sublimation
absorbs (in atomic spectra)


36. When solids are heated at certain perssures - some solids vaporize directly without passing through the liquid phase.
sublimation
emits (in atomic spectra)
combination
partial


37. Increase in the concentrations of reactants shifts the equilibrium to the ______ - thus increasing the amount of products formed.

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38. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
high
molar heat of sublimation
left (Le Chatelier's principle)
heats of formation


39. In an endothermic process - energy is absorbed and ^E is _______.
bohr model
ideal gas
positive
second law of thermodynamics


40. 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.
kinetic molecular theory
first law of thermodynamics
upper right corner
...


41. 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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42. 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.
heats of formation
Van der Waals
reversible reaction
system (thermodynamics)


43. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
positive charge
decreases
right (Le Chatelier's principle)
second law of thermodynamics


44. A catalyst affects a chemical reaction by lowering the _____ _____ for both the forward and the reverse reactions equally.
reversible reaction
phase equilibrium
activation energy
base - acid


45. The most active metals are found in what corner of the periodic table?
lower left corner
sublimation
third law of thermodynamics
upper right corner


46. The change in enthalpy of an exothermic reaction is ________.
limiting law
negative
equivalent point
electronegativity


47. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
emits (in atomic spectra)
partial
specific heat
moles (Le Chatelier's principle)


48. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
Van der Waals
Boyles law
upper right corner
positive


49. The pressure exerted by each gas in a mixture is called its _____ pressure.
ionization energy
partial
irreversible and reversible processes
combined gas law


50. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
standard atmospheric pressure
Charles law
limiting law
positive