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College > CH302 Exam 4 > Flashcards

CH302 Exam 4 Flashcards

1
Q

Oxidation Agent

A

Molecule being reduced

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2
Q

Reduction agent

A

molecule being oxidized

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3
Q

Activity series: lower on chart…

A

G decreases, harder to oxidize, more stable

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4
Q

Activity series: higher on chart…

A

G increases, easier to oxidize, less stable

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5
Q

salt bridge

A

keeps charge neutral

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6
Q

Reduction

A

Gains electrons on left side of 0.5 eqn

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7
Q

Oxidation

A

Loses electrons on right side of 0.5 eqn

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8
Q

Agents are in left or right side?

A

Left

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9
Q

In a working electrochemical cell (a voltaic or a battery), the cations in the salt bridge move toward the cathode.

A

True

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10
Q

Voltage for Voltaic Cell

A

Anode - Cathode

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11
Q

Voltage for Elctrolytic Cell

A

Cathode - Anode

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12
Q

Strongest Reducing Agent?

A

Li

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13
Q

Oxidation and reduction take place at the same time, but at different electrodes in a…

A

voltaic cell

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14
Q

A discharging battery is a voltaic cell, meaning it’s…

A

Spontaneous with a positive cell potential

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15
Q

Suppose you set up an electrochemical cell. In one beaker, you have a 1 M copper(II) ion solution with a copper metal electrode. You use an external wire to connect the copper electrode to an aluminum electrode in another beaker with a 1 M aluminum ion solution. Then you add a salt bridge with sodium sulfate ions. All things are in place to have a functional cell. Which of the following statements is FALSE?

A

Nothing will happen until you add an external power source

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16
Q

What’s the purpose of Pt?

A

Pt is an inert electrode used to conduct electrons into the external circuit

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17
Q

Why might you use an inert electrode in your standard cell set-up?

A

Half-rxn doesn’t include a solid state conductor

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18
Q

One faraday =

A

total charge on one mole of electrons

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19
Q

Consider the following cell that is set up at standard conditions:

Cu | Cu2+ (1 M) || Cu2+ (1 M) | Cu

If you were to increase the copper ion concentration in the cathode compartment, what would happen to the overall cell potential (E)?

A

the overall potential will increase slightly becoming positive

20
Q

A concentration cell is made by putting two Ag+ solutions in separate beakers and connecting them with a wire and a salt bridge. The cathode has a concentration of 3.80 M and the anode has a concentration of 0.0150 M. What type of cell is this at these nonstandard conditions?

A

voltaic

21
Q

You are examining a non-rechargeable D-cell battery that you are about to put in a flashlight. You see that one end is labeled + and the other is labeled – . Now that you have studied batteries, you know that the + indicates the end of the battery that is the:

A

cathode

22
Q

You turn on a flashlight containing brand new NiCad batteries and keep it lit for a minute or two. Which of the following can be considered TRUE regarding the chemical state of these batteries?

I. The chemical reaction is spontaneous

II. Ecell > 0

III. The overall redox reaction in the battery is at equilibrium

IV. Ecell is substantially decreasing during this time

A

I and II

23
Q

A primary battery is

A

a voltaic cell

24
Q

A secondary cell can be

A

voltaic cell, electrolytic cell, and recharged

25
Q

What metal (in various oxidation states) is present at both the cathode and the anode in a typical car battery?

A

Lead

26
Q

You start you car and begin driving. After about 10 to 15 minutes of driving your car just dies and will not restart. Which of the following reasons is the most logical explanation why your car died?

A

The alternator is not properly recharging the battery as you are driving

27
Q

A secondary battery that is discharging is running a ________ chemical reaction and a secondary battery that is recharging is running a _________ chemical reaction.

A

spontaneous, nonspontaneous

28
Q

The common alkaline cell batteries (D, AA, AAA, etc.) share the same voltage but differ on the basis that…

A

The maximum current that can be delivered is proportional to the surface area of the electrodes - so the bigger battery sizes are able to deliver more current.

29
Q

The net redox reaction in a fuel cell is given below:

2H2 + O2 —> H2O

What is the reaction at the anode in a fuel cell?

A

H2 —> 2H+ + 2e–

30
Q

It is not a good idea to make a battery out of standard conditions (1 M of all aqueous products). Instead, you can modify the concentrations so that…

A

Q < 1 and E_cell > E`_cell

31
Q

Which of the following batteries are rechargeable?

I. alkaline battery

II. NiMH battery

III. lithium battery

IV. Li-ion battery

V. Pb-acid battery

A

II, IV, and V only

32
Q

Nernst Eqn

A

E = E- (0.05916/n) * log Q (look out for coeff.) OR E = E- (0.0257/n) * ln Q

33
Q

Q =

A

Anode / Cathode

34
Q

Work Eqn.

A

deltaG = -nFE

35
Q

Voltaic Cell List

A

deltaG and anode is (-). E and cathode is (+)

36
Q

Electrolytic Cell List

A

deltaG and anode is (+). E and cathode is (-)

37
Q

Spontaneous

A

K > 1 and products favored

38
Q

Non-spontaneous

A

K < 1 and reactants favored

39
Q

Potential and equil. Constant Eqn

A

logK = nE`/0.0591

40
Q

Ksp eqn.

A

= exp(nFE/RT)

41
Q

Fuel Cells

A

Refillable

42
Q

Car battery

A

Either voltaic or electrolytic cell depending on whether it’s charging or not

43
Q

Here is the discharge reaction for an alkaline battery:

Zn(s) + 2MnO2(s) + H2O(l) —–> Zn(OH)2(s) + Mn2O3(s)

Which species is reduced as the battery is discharged?

A

MnO2(s)

44
Q

SHE

A

consists Pt wire that’s connected to Pt surface (E` = 0)

45
Q

Secondary cell examples

A

NiMH, NiCad, lead based, lithium ion

46
Q

Primary cells examples

A

Alkaline battery, lithium cells, silver oxide, dry cell, zn-c

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