PhyChem 2 Midterm Exam Flashcards

1
Q

Mixtures for which the solute obeys Henry’s law and the solvent obeys Raoult’s law are called ___________________.

A

ideal-dilute solutions

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2
Q

The ratio of the partial vapour
pressure of each component to its vapour pressure as a pure liquid, pA/p*A, is approximately equal to the mole fraction of A in the liquid mixture.

A

Raoult’s law

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3
Q

for real solutions at low concentrations, although the vapour pressure of the solute is proportional to its mole fraction, the constant of proportionality is not the vapour pressure of the pure substance.

A

Henry’s Law

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4
Q

A ________________ depends only on the number of solute particles present, not
their identity.

A

colligative property

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5
Q

Enumerate the colligative properties.

A

(a) elevation of boiling point
(b) depression of the freezing point
(c) solubility
(d) osmosis

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6
Q

(from the Greek word for ‘push’) is the spontaneous passage of a pure solvent into a solution separated from it by a semipermeable membrane

A

osmosis

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7
Q

The _____________ theory ascribes deviations from ideality to the Coulombic interaction of an ion with the ionic atmosphere that assembles around it.

A

Debye–Hückel

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8
Q

delta G<0, (exergonic) the forward reaction is

A

spontaneous

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9
Q

delta G>0, (endergonic) reverse reaction is

A

spontaneous

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10
Q

delta G=0, reaction is

A

equilibrium

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11
Q

A system at equilibrium, when subjected to a disturbance, responds in a way that tends to minimize the effect of the disturbance

A

Le Chatelier’s principle

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12
Q

__________________ is an expression for the slope of a plot of the equilibrium constant (specifically, ln K) as a function of
temperature

A

van’t Hoff equation

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12
Q

E* is also known as the ______________.

A

standard electrode potential

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13
Q

Oxidation is ________ of electrons.

A

loss

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14
Q

Reduction is ________ of electrons.

A

gain

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15
Q

Oxidation and reduction occur __________.

A

simultaneously

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16
Q

Oxidation results in an ________ in oxidation number.

A

increase

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17
Q

Reduction results in an ________in oxidation number.

A

decrease

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18
Q

Zn to Zn+2 is ____________ because___________.

A

oxidation because the O.N increases from 0 to +2

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19
Q

H+ to H is ____________ because_________________.

A

reduction because the O.N decreases from +1 to 0.

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20
Q

If delta G<0 then the reaction is ___________.

A

spontaneous

21
Q

a _________________ uses a spontaneous redox reaction to generate electrical energy.

A

voltaic cell

22
Q

a ________________ uses electrical energy to drive a nonspontaneous reaction.

A

electrolytic cell

23
Q

delta G>0 then the reaction is _________.

A

nonspontaneous

24
Electrochemical cells are constructed using 2 main components ____________ and ____________ solution.
electrolyte and electrode
25
The electrode at which oxidation occurs.
anode
26
The electrode at which reduction occurs.
cathode
27
It is a cell where energy is released from a spontaneous redox reaction.
voltaic cell
28
It is a cell where energy is absorbed to drive a nonspontaneous redox reaction.
electrolytic cell
29
electrons flow from __________ to ______________.
anode to cathode
30
half cells are connected by the external circuit that is called ___________.
salt bridge
31
Anode is the __________ electrode in a voltaic cell.
negative
32
Cathode is the __________ electrode in a voltaic cell.
positive
33
Salt bridge allows ________ to flow through both half cells.
ions
34
The salt bridge maintains ___________ __________ by allowing excess Zn2+ ions to enter from the anode, and excess negative ions enter from the cathode.
electrical neutrality
35
A salt bridge contains ____________ cations and anions often K+ and NO3-; dissolved in a gel.
nonreacting
36
_____________ electrode is a component in its half cell and is a reactant or product in the overall reaction.
active
37
_____________ electrode provides a surface for the reaction and completes the circuit. It does not participate actively in the overall reaction.
inactive
38
Name 2 examples of common inactive electrodes.
Platinum and graphite
39
Anode components are written on the _________________.
left
40
Cathode components are written on the _________________.
right
41
double line in a cell notation means ____________.
half cells are physically separated.
42
the single line shows a _________ between the components of a half cell.
phase boundary
43
a comma is used to show that _____________.
components are in the same phase.
44
It depends on the difference in electrical potential between the two electrodes.
cell potential
45
the cell potential is also known as the _______________ or ____________________.
voltage of the cell or the electromotive forces (emf)
46
The ______________ is designated Ecell and is measured at a specific temperature with no current flowing and all components in their standard states.
Standard Cell Potential
47
Ecell is equal to (write the formula)
Ecell= cathode minus anode
48
___________________ has a standard electrode potential defined as 0.
Standard Hydrogen Electrode
49
potential rises due to a chemical reaction occurring in the cell
Chemical cell
50
potential rises due to a concentration difference, resulting in transfer of matter.
Concentration cell