EXAM 4 Flashcards
Reduction is the
gain of electrons.
loss of electrons.
gain of protons.
loss of protons.
loss of mass.
Oxidation is the
gain of electrons.
loss of electrons.
gain of protons.
loss of protons.
loss of mass.
loss of electrons
What is the oxidation number of chromium in the ionic compound ammonium dichromate, (NH4)2Cr2O7?
+3
+4
+5
+6
+7
+6
On a periodic table, where do you expect to find elements that are good oxidizing agents?
on the right (except for the last group)
in the middle left
in the top left
at the bottom
in the transition metals
on the right (except for the last group)
Where in the periodic table do you find the elements that are the best reducing agents with the most negative standard reduction potentials?
in group 16
on the left
in the middle
at the bottom
in group 17
on the left
Applying a current to a rechargeable battery converts it from ________ cell to ________ cell.
a voltaic; an electrolytic
an electrolytic; a voltaic
a Leclanché; a Nernst
a Nernst; a Leclanché
a Born cell; a Haber
a voltaic; an electrolytic
Which statement is correct about a voltaic cell?
The electron flow in the external circuit is from the positive electrode to the negative electrode.
The electron flow in the external circuit is from the cathode to the anode.
Electrons are transferred from the oxidizing agent to the reducing agent.
Chemical energy is transformed into electrical energy by a spontaneous redox reaction.
Positive ions diffuse through a porous bridge from the cathode compartment to the anode compartment.
Chemical energy is transformed into electrical energy by a spontaneous redox reaction.
Which statement about an anode in a voltaic cell is correct?
Oxidation occurs at the anode.
Reduction occurs at the anode.
Usually, the cathode is a dissolved ion.
In the external circuit, electrons flow toward the anode.
Chemical species can have their oxidation numbers decreased at the anode.
Oxidation occurs at the anode.
The electrodes on batteries are labeled + and -. The ________ is labeled ________, and ________ occurs there.
anode; positive; oxidation
anode; negative; reduction
cathode; positive; reduction
cathode; negative; reduction
cathode; positive; oxidation
cathode; positive; reduction
The electrodes on batteries are labeled + and -. The ________ is labeled ________, and ________ occurs there.
anode; positive; oxidation
anode; negative; oxidation
cathode; positive; oxidation
cathode; negative; reduction
anode; positive; reduction
anode; negative; oxidation
This diagram represents a voltaic cell. In this cell, which species is oxidized?
Cd(s)|Cd2+ (aq)||Fe3+ (aq),Fe2+ (aq)|Pt(s)
Cd(s)
Cd2+ (aq)
Fe2+ (aq)
Fe3+ (aq)
Pt(s)
Cd(s)
This diagram represents a voltaic cell. In this cell, which species is reduced?
Zn(s)|Zn2+ (1.0 M)||Cu2+ (1.0 M)|Cu(s)
Zn(s)
Zn2+ (aq)
Cu2+ (aq)
Cu(s)
C(s)
Cu2+ (aq)
This diagram represents a voltaic cell. What is the balanced electrochemical reaction represented by this cell?
Al(s)|Al3+ (1.0 M)||Cu2+ (1.0 M)|Cu(s)
2Al(s) + 3Cu2+(aq) 2Al3+(aq) + 3Cu(s)
2Al3+(aq) + 3Cu(s) 2Al(s) + 3Cu2+(aq)
2Al(s) + 3Cu2+(aq) 2Al3+(aq) + 3Cu(s)
This diagram represents a voltaic cell. In this cell, which species is the oxidizing agent?
Al(s)|Al3+ (1.0 M)||Cu2+ (1.0 M)|Cu(s)
Cu2+ (aq)
Cu(s)
Al(s)
Al3+ (aq)
Pt(s)
Cu2+ (aq)
If the potential of a voltaic cell is +1.20 V, what is the free-energy change when one mole of electrons is transferred in the oxidation–reduction reaction?
116 kJ
1.20 kJ
-1.20 kJ
-116 kJ
+602 kJ
-116 kJ
If the potential of a voltaic cell is +0.837 V, what is the free-energy change when two moles of electrons are transferred in the oxidation–reduction reaction?
+162 kJ
-162 kJ
-82.0 kJ
+82.0 kJ
+41.0 kJ
-162 kJ
The spontaneous redox reaction in a voltaic cell has
a negative value of Ecell and a negative value of ΔG.
a positive value of Ecell and a positive value of ΔG.
a negative value of Ecell and a positive value of ΔG.
a positive value of Ecell and a negative value of ΔG.
a positive value of Ecell and a value of zero for ΔG
a positive value of Ecell and a negative value of ΔG.
The standard hydrogen electrode is
used to calibrate voltmeters.
used to produce a set of standard reduction potentials.
needed to activate electrochemical cells.
often overlooked in measuring standard reduction potentials.
used to produce a standard cell potential of exactly 1 V.
used to produce a set of standard reduction potentials.
The Nernst equation can be used to calculate
standard cell potentials from standard reduction potentials.
the change in standard Gibbs free energy from standard cell potentials.
cell potentials from standard cell potentials when the conditions of concentration and temperature are not standard.
cell potentials given the temperature and reactant concentrations.
cell potentials from standard oxidation potentials.
cell potentials from standard cell potentials when the conditions of concentration and temperature are not standard.
A concentration cell is constructed by using the same half-reaction for both the cathode and anode. What is the value of standard cell potential, , for a concentration cell that combines a silver anode in contact with 0.10 M silver nitrate and a silver cathode in contact with 0.00003 M silver nitrate? ( Ered=+0.80 V for Ag/Ag+)
-0.21 V
0.00 V
+0.80 V
-0.80 V
+0.21 V
0.00V
Which statement correctly describes a “dead” battery with a voltage of 0?
The free-energy change for the reaction now is < 0.
All the reactants have been converted into products.
The products and reactants now are in equilibrium.
Q<K
cell potential < 0
The products and reactants now are in equilibrium.
What is true when a battery (voltaic cell) is dead?
Ecell= 0 and Q=K
Ecell= 0 and Q=K
Ecell= 0 and Q= 0
Ecell = 0 and Q= 0
Ecell= 0 and K= 0
Ecell= 0 and Q=K
A concentration cell is constructed by using the same half-reaction for both the cathode and anode. What is the value of Ecell for a concentration cell that combines silver electrodes in contact with 0.10 M silver nitrate and 0.00003 M silver nitrate solutions? ( Ered=+0.80 V for Ag/Ag+)
+0.21 V
+0.59 V
+0.80 V
-0.21 V
+1.01 V
+0.21V
A typical 1.5 V AAA battery has a capacity of 1 ampere-hour (A × hr.). How much energy can such a battery supply?
5400 J
1.5 J
3600 J
1800 J
90 J
5400 J
A typical hearing aid battery has a capacity of 5 ampere-hour (A × hr.) and can supply up to 23.4 kJ of energy. What is the voltage of the battery?
78 V
1.3 V
1.3 × 10-3 V
7.8 × 10-3 V
0.90 V
1.3 V
What is the mass of copper used if it was oxidized to copper(II) over 35.0 s, given the average electrical current delivered was 200. A?
1.02 × 10-1 g
1020 g
2.30 g
4.60 g
1.00 g
2.30 g