NEW
Font size
S
M
L
XL
WorksheetsRedox 1: Galvanic Cells
Total questions: 9
Worksheet time: 45mins
Name
Class
Date
1.
Consider the galvanic cell given.
Which of the following deductions about this cell is correct?
Which of the following deductions about this cell is correct?
a)
Oxidation is occurring in half-cell 2
b)
The positive electrode is in half-cell 2
c)
Oxidation is occurring in half-cell 1
d)
The negative electrode is in half-cell 1
2.
Consider the galvanic cell represented, operating at 25oC , 101.3 kPa and using 1 M solutions.
The product(s) of the half-reaction occurring in half-cell 1 is (are)
The product(s) of the half-reaction occurring in half-cell 1 is (are)
a)
Ni (s)
b)
Ni2+ (aq)
c)
H2O2 (aq)/H+ (aq)
d)
H2O (l)
3.
A galvanic cell is established to power a torch, as shown.
For this cell, the
For this cell, the
a)
electrons will flow from the aluminium to the hydrogen half-cell
b)
aluminium electrode will be the positive anode
c)
concentration of aluminium ions in solution will be falling
d)
hydrogen half-cell will be the negative cathode
4.
A galvanic cell is established to power a torch, as shown.
For this cell, the overall equation will be
For this cell, the overall equation will be
a)
2Al(s)+3H2(g)→2Al3+(aq)+6H+(aq)
b)
3Cl-(aq)+Al(s)→AlCl3(aq)
c)
2Al3+(aq)+3H2(g)→2Al(s)+6H+(aq)
d)
2Al(s)+6H+(aq)→2Al3+(aq)+3H2(g)
5.
A VCE chemistry student sets up a galvanic cell using two standard half-cells with half reactions.
Half-cell 1: Cr3+(aq)+e-→Cr2+(aq)
Half-cell 2: Cr(s)→Cr2+(aq)+2e-
Sutable materials for the electrodes of te two half-cells are
Half-cell 1: Cr3+(aq)+e-→Cr2+(aq)
Half-cell 2: Cr(s)→Cr2+(aq)+2e-
Sutable materials for the electrodes of te two half-cells are
a)
Half-cell 1: Platinum; Half-cell 2: Platinum
b)
Half-cell 1: Platinum; Half-cell 2: Chromium
c)
Half-cell 1: Chromium; Half-cell 2: Chromium
d)
Half-cell 1: Chromium; Half-cell 2: Platinum
6.
The experimental arrangement shows a:
- silver rod dipping into a 1.0 M solution of AgNO3 (aq)
- nickel rod dipping into a 1.0 M solution of Ni(NO3)2 (aq)
The solutions are connected to each other with a salt bridge consisting of an inverted U-tube containing ammonium nitrate solution.
Which of the following alternatives correctly describes the polarity of, and the reaction that occurs at, the anode of this cell?
- silver rod dipping into a 1.0 M solution of AgNO3 (aq)
- nickel rod dipping into a 1.0 M solution of Ni(NO3)2 (aq)
The solutions are connected to each other with a salt bridge consisting of an inverted U-tube containing ammonium nitrate solution.
Which of the following alternatives correctly describes the polarity of, and the reaction that occurs at, the anode of this cell?
a)
Negative; Ag+(aq)+e-→Ag(s)
b)
Negative; Ni(s)→Ni2+(aq)+2e-
c)
Positive; Ag+(aq)+e-→Ag(s)
d)
Positive; Ni(s)→Ni2+(aq)+2e-
7.
A galvanic cell consists of one half-cell that is made up of an inert graphite electrode in a solution containing 1.0 M Fe2+ (aq) and 1.0 M Fe3+ (aq) at 25oC. Which one of the following could be used as the second half-cell so that the polarity of the electrode in this second half-cell is positive?
a)
a lead electrode in a solution of 1.0 M Pb2+ (aq)
b)
a silver electrode in a solution of 1.0 M Ag+ (aq)
c)
an iron electrode in a solution of 1.0 M Fe2+ (aq)
d)
an inert graphite electrode in a solution of 1.0 M Br- (aq)
8.
Two standard galvanic cells are shown.
On the basis of the polarity of the electrodes shown, which one of the following reactions would NOT be expected to occur spontaneously?
On the basis of the polarity of the electrodes shown, which one of the following reactions would NOT be expected to occur spontaneously?
a)
Co2+(aq)+Cd(s)→Co(s)+Cd2+(aq)
b)
2Mn3+(aq)+Co(s)→2Mn2+(aq)+Co2+(aq)
c)
2Mn3+(aq)+Cd(s)→2Mn2+(aq)+Cd2+(aq)
d)
2Mn2+(aq)+Co2+(aq)→2Mn3+(aq)+Co(s)
9.
Two galvanic cells were constructed under standard conditions in an experiment to determine the relative positions in the electrochemical series of the standard electrode potential, Eo, for the following reactions. Both cells generate a potential difference.
Ag(NH3)2+(aq) + e-↔ Ag(s) + 2NH3(aq); Eo1
Ag+(aq) + e-↔ Ag(s); Eo2
Ag(CN)-2(aq) + e-↔ Ag(s) + 2CN- (aq); Eo3
The values of the electrode potentials in order from highest to lowest would be
Ag(NH3)2+(aq) + e-↔ Ag(s) + 2NH3(aq); Eo1
Ag+(aq) + e-↔ Ag(s); Eo2
Ag(CN)-2(aq) + e-↔ Ag(s) + 2CN- (aq); Eo3
The values of the electrode potentials in order from highest to lowest would be
a)
Eo1; Eo2; Eo3
b)
Eo1; Eo3; Eo2
c)
Eo2 ;Eo1; Eo3
d)
Eo3; Eo2 ;Eo1
Reset
