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. The heat required to change 1mole of solid completely to vapor.
molar heat of sublimation
combined gas law
irreversible and reversible processes
Charles law


2. A state function in which it is the heat content of a substance.
enthalpy
increasing
high
kinetic molecular theory


3. The amount of heat energy required to raise the temperature of a given quantity of a substance one degree celcius.
ionization energy
activation energy
heat capacity
Van der Waals


4. A law stating that at constant pressure - the volume of a given quantity of a gas varies directly with the temperature.
enthalpy
decomposition
upper right corner
Charles law


5. 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.
Raoults law
Le Chatelier's principle
bohr model
titration


6. 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 _____ _
wave mechanical model
emits (in atomic spectra)
limiting law
decreases


7. 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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8. 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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9. 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).
boiling point elevation
isothermal process (thermodynamics)
Van der Waals
sublimation


10. The solubility of gases in liquid or solid solvents always increases with ________ pressure.
increasing
wave mechanical model
increases
Charles law


11. A pure crystal of elemental metal consists of roughly Avogrado's number of atoms held together by ________ bonds.
valence
specific heat
total pressure (Le Chatelier's principle)
metallic


12. A hypothetical gas would follow Boyles law under all conditions and is called?
wave mechanical model
ionization energy
ideal gas
bohr model


13. The vapor pressure of an aqueous solution is always lowered by the additon of more solute - which causes the boiling point to be raised.
system (thermodynamics)
ionization energy
boiling point elevation
equilibrium


14. This law states that the entropy of any pure - perfect crystal at absolute zero is equal to zero.
kinetic molecular theory
Boyles law
saturated solution
third law of thermodynamics


15. The law stating that in any spontaneous process there is an increase in the entropy of the universe.
second law of thermodynamics
absorbs (in atomic spectra)
double replacement/displacement
increases


16. The particular portion of the universe on which we wish to focus our attention. Everything else is called the surroundings.
first law of thermodynamics
Valence Shell Electron Pair Repulsion (VSEPR)
electrolytic reactions
system (thermodynamics)


17. **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.
...
Boyles law
adiabatic process (thermodynamics)
decreases


18. A law that states that for a given mass of gas - the volume is proportional to the pressure and absolute temperature.
combined gas law
10 degrees
irreversible and reversible processes
limiting law


19. 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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20. A chemical reaction formed from the breakdown of a compound into its individual elements or compounds.
...
decomposition
boiling point elevation
negative


21. This process occurs when the system is thermally isolated so that no heat enters or leaves.
Nernst equation
adiabatic process (thermodynamics)
colligative property law
ideal gas


22. 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.
equivalent point
emits (in atomic spectra)
decreases
standard atmospheric pressure


23. 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.
decomposition
VSEPR
equilibrium
Van der Waals


24. The enthalpy changes associated with the reactions that correspond to the formation of a substance from its free elements are called?
Van der Waals
heats of formation
Charles law
state (thermodynamics)


25. When the electron moves from the ground state to an excited state - it ______ energy.
catalysts
reversible reaction
Le Chatelier's principle
absorbs (in atomic spectra)


26. A chemical reaction formed from the union of its elements.
system (thermodynamics)
combination
irreversible and reversible processes
equilibrium


27. 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
reversible reaction
pi bonds
double replacement/displacement


28. The temperature at which a substance's solid and liquid phases are in equilibrium.
melting point
adiabatic process (thermodynamics)
wave mechanical model
zero


29. The force with which the electrons flow from the negative electrode to the positive electrode through an external wire is called?
specific heat
Daltons law
electromotive force (emf)/ cell
Charles law


30. The normal boiling point of a liquid is the temperature at which its vapor pressure is 760mm Hg.
Nernst equation
ideal gas
standard atmospheric pressure
heats of formation


31. 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.
temperature
wave mechanical model
state functions (thermodynamics)
Le Chatelier's principle


32. Metals have electronegativities less than ____
pressure
2
third law of thermodynamics
lower left corner


33. A chemical reaction where one substance is displacing another. ex: Fe + CuSo4 -> FeSo4 + Cu.
kinetic molecular theory
increases
single replacement/displacement
saturated solution


34. Electronegativities _______ as you go down a group.
decreases
enthalpy
pi bonds
point particles


35. Any spontaneous change in a chemical reaction will decrease the amount of free energy toward _______ as the process proceeds towards equilibrium.
irreversible and reversible processes
Le Chatelier's principle
single replacement/displacement
zero


36. When a hydrogen atom is bonded to a highly electronegative atom - it will become partially _____-charged - and will be attracted to neighboring electron pairs. This creates a hydrogen bond. The more polar the molecule - the more effective the hydroge
freezing point depression
phase equilibrium
positive charge
moles (Le Chatelier's principle)


37. 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
positive charge
state functions (thermodynamics)
10 degrees


38. Gases are composed of tiny - invisible molecules that are widely separated from one another in otherwise empty space.
combined gas law
reversible reaction
kinetic molecular theory
single replacement/displacement


39. The amount of heat energy required to raise the temperature 1g of a substance by 1 degree celcius.
specific heat
temperature
Van der Waals
Raoults law


40. Another way the second law is stated is that in any spontaneous change - the amount of free energy available ______.
heat capacity
decreases
electromotive force (emf)/ cell
specific heat


41. 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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42. *The surface area exposed affect chemical reactions because most reactions depend on the reactants coming into contact - increasing the rate of the reaction.
left - right (Le Chatelier's principle)
...
second law of thermodynamics
Charles law


43. Reactions that do not occur spontaneously can be forced to take place by supplying energy with an external current.
positive
electrolytic reactions
Charles law
base - acid


44. *The nature of the reactants and products affect chemical reactions because some elements and compounds have bonds that when broken/formed - react more rapidly with each other than others.
hybridyzation
right (Le Chatelier's principle)
left (Le Chatelier's principle)
...


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. The vapor pressure increases with increasing _____.
10 degrees
lower left corner
dynamic equilibrium
temperature


47. *Molecules of ideal gases have no attraction for one another and have no intrinsic volume - they are ______ _____
Valence Shell Electron Pair Repulsion (VSEPR)
upper right corner
point particles
right (Le Chatelier's principle)


48. Rays made up of positive electrodes in basic electron charges.
point particles
Van der Waals
anode rays
dynamic equilibrium


49. The pressure exerted by the gas molecules when they are in equilibrium with the liquid.
left - right (Le Chatelier's principle)
vapor pressure
partial
decreases


50. The molecules in a gas collide with one another - but the collisions are perfectly elastic (they result in no net loss of energy).
right (Le Chatelier's principle)
Van der Waals
positive
kinetic molecular theory