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. 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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2. A process that occurs whent eh system is maintained at constant pressure.
isopiestic process (thermodynamics)
activation energy barrier (Le Chatelier's principle)
boiling point
molar heat of sublimation


3. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
positive charge
first law of thermodynamics
equivalent point


4. A state function in which it is the heat content of a substance.
Nernst equation
standard atmospheric pressure
melting point
enthalpy


5. A law that states that under conditions of constant temperature and pressure - equal volumes of different gases contain equal numbers of molecules.
single replacement/displacement
heats of formation
Avogrados law
entropy


6. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
Charles law
irreversible and reversible processes
kinetic molecular theory
Daltons law


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

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8. The temperature at which a substance's solid and liquid phases are in equilibrium.
...
increases
partial
melting point


9. 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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10. For most substances - when a hot concentrated solution is cooled - the excess solid ________. This is useful in purification of the solute.
single replacement/displacement
decreases
crystallizes
non-ideal


11. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
reversible
right (Le Chatelier's principle)
limiting law
increasing


12. When the rate of evaporation equals the rate of condensation - the system is in __________.
kinetic molecular theory
heats of formation
equilibrium
isothermal process (thermodynamics)


13. The change in enthalpy of an endothermic reaction is ________.
positive charge
positive
bohr model
limiting law


14. _____ bonds are present in molecules containing double or triple bonds.
point particles
pi bonds
ideal gas
phase equilibrium


15. 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.
Valence Shell Electron Pair Repulsion (VSEPR)
saturated solution
colligative property law
Boyles law


16. This process occurs when the system is thermally isolated so that no heat enters or leaves.
electrolytic reactions
adiabatic process (thermodynamics)
cathode rays
zero


17. 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 _____ _
irreversible and reversible processes
positive
negative
limiting law


18. The pressure exerted by each gas in a mixture is called its _____ pressure.
partial
negative
dynamic equilibrium
point particles


19. 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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20. The energy required to remove an electron from an isolated atom in its ground state.
Raoults law
ionization energy
Van der Waals
high


21. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
decreases
metallic
pressure
bohr model


22. 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.
increases
Boyles law
Raoults law
freezing point depression


23. 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)
Van der Waals
combination
positive


24. The relatively weak attractive forces between molecules that are apparent only when the molecules approach one another closely (usually at low temperatures and high pressure).
Van der Waals
...
moles (Le Chatelier's principle)
kinetic molecular theory


25. The most active metals are found in what corner of the periodic table?
heat capacity
decreases
lower left corner
Le Chatelier's principle


26. Electronegativities _______ as you go down a group.
decreases
lower left corner
decomposition
kinetic molecular theory


27. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
single replacement/displacement
total pressure (Le Chatelier's principle)
molar heat of sublimation
crystallizes


28. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
double replacement/displacement
metallic
Daltons law
heat capacity


29. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
vapor pressure
lower left corner
Boyles law
dynamic equilibrium


30. The heat change during a process carried out at a constant pressure.
kinetic molecular theory
change in enthalpy
...
heat capacity


31. In a _______ expansion of a gas - the opposing pressure is virtually equal to the pressure exerted by the gas. It is ______ because any slight increase in the external pressure will reverse the process and cause compression to occure.
reversible
zero
combination
melting point


32. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
freezing point depression
specific heat
activation energy barrier (Le Chatelier's principle)
isothermal process (thermodynamics)


33. **Proceeding across a period from left to right - the ionization energy _______.
kinetic molecular theory
Raoults law
combination
increases


34. The process of mixing different orbitals of the same atom to form a new set of equivalent orbitals.
VSEPR
single replacement/displacement
irreversible and reversible processes
hybridyzation


35. This process occurs when the system is maintained at the same temperature throughout an experiment.
isothermal process (thermodynamics)
moles (Le Chatelier's principle)
colligative property law
hybridyzation


36. 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
reversible reaction
third law of thermodynamics


37. 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.
titration
pressure
end point
non-ideal


38. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
point particles
positive
crystallizes
isopiestic process (thermodynamics)


39. **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.
catalysts
...
activation energy barrier (Le Chatelier's principle)
kinetic molecular theory


40. 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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41. A solution in which solid solute is in equilibrium with dissolved solute.
positive
freezing point depression
enthalpy
saturated solution


42. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
increases
electromotive force (emf)/ cell
sublimation
kinetic molecular theory


43. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
heats of formation
equivalent point
kinetic molecular theory
saturated solution


44. 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.
hydrolysis
electronegativity
wave mechanical model
Van der Waals


45. *The temperature affects chemical reactions with an increase of ___degrees C above room temperature - causing the reaction rate to double.
...
10 degrees
moles (Le Chatelier's principle)
titration


46. A law stating that at a constant temperature - the volume of a gas in inversely proportiona to the pressure.
end point
melting point
phase equilibrium
Boyles law


47. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
2
hybridyzation
state functions (thermodynamics)
boiling point elevation


48. Heat added to a system and work done by a system are considered _________ quantities.
kinetic molecular theory
boiling point
positive
isopiestic process (thermodynamics)


49. 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.
Avogrados law
valence
electronegativity
increases


50. _______ has very little effect on the solubility of liquids or solids in liquid solvents.
catalysts
increases
pressure
ideal gas