NEW
Font size
S
M
L
XL
WorksheetsSalad Quiz 6
Total questions: 9
Worksheet time: 45mins
Name
Class
Date
1.
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)
2.
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)
3.
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
4.
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-
5.
The strongest reducing agent from the following list: Fe3+; Sn2+; H2O; K+; Br-; Au; Pb2+ is
a)
K+
b)
Fe3+
c)
Sn2+
d)
Au
6.
Three half-cells were set up under standard conditions:
Half-cell 1: Electrode = Graphite; Electrolyte=P2+(aq) and P3+(aq)
Half-cell 2: Electrode = Metal Q; Electrolyte=Q2+(aq) Half-cell 3: Electrode = Metal R; Electrolyte=R2+(aq)
Two galvanic cells were constructed using combinations of these half-cells. The results obtained are shown in the table given. Based on these results, which of the following is the strongest reducing agent?
Half-cell 1: Electrode = Graphite; Electrolyte=P2+(aq) and P3+(aq)
Half-cell 2: Electrode = Metal Q; Electrolyte=Q2+(aq) Half-cell 3: Electrode = Metal R; Electrolyte=R2+(aq)
Two galvanic cells were constructed using combinations of these half-cells. The results obtained are shown in the table given. Based on these results, which of the following is the strongest reducing agent?
a)
P2+(aq)
b)
P3+(aq)
c)
R(s)
d)
Q(s)
7.
Hydrogen peroxide can act as a reductant to the half-equation:
O2 (g) + 2H+(aq) + 2e- → H2O2(aq); Eo=+0.68 V
Which of the following could be reduced by hydrogen peroxide?
O2 (g) + 2H+(aq) + 2e- → H2O2(aq); Eo=+0.68 V
Which of the following could be reduced by hydrogen peroxide?
a)
Fe2+(aq); Cu(s); I-(aq)
b)
Ag+(aq); Br2(aq); H2O2(aq)
c)
Ag(s); Br-(aq); Fe2+(aq)
d)
I2(s); Cu2+(aq); Fe3+(aq)
8.
Bomb calorimeters may be calibrated by combusting a pure substance with a known heat of combustion. A particular bomb calorimeter was calibrated using 100mL of pure ethanol (density 0.789 g mL-1). If the temperature rose by 10.4oC during the combustion of pure ethanol, the calibration factor for the calorimeter would be
a)
131 kJ oC-1
b)
197 kJ oC-1
c)
226 kJ oC-1
d)
285 kJ oC-1
9.
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
Reset
