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WorksheetsA level electrochemical cells
Total questions: 10
Worksheet time: 35mins
Name
Class
Date
1.
he standard redox potentials for a number of substances are shown below:
F2(g) + 2e-→ 2F-(aq); E0 = 2.87 V
O2(g)+ 4H+(aq)+ 4e-→ 2H2O(l); E0 = 1.23 V
Cu2+(aq) + 2e-→ Cu(s); E0 = 0.34 V
Fe2+(aq) + e- → Fe(s); E0 = -0.41V
2H2O(l) + 2e- → H2(g) + 2OH-(aq); E0 = -0.83 V
Mg2+(aq) + 2e- → Mg(s); E0 = -2.38 V
If all of these substances were available, what galvanic cell could be set up using these substances that would steadily deliver approximately 1.6 V?
F2(g) + 2e-→ 2F-(aq); E0 = 2.87 V
O2(g)+ 4H+(aq)+ 4e-→ 2H2O(l); E0 = 1.23 V
Cu2+(aq) + 2e-→ Cu(s); E0 = 0.34 V
Fe2+(aq) + e- → Fe(s); E0 = -0.41V
2H2O(l) + 2e- → H2(g) + 2OH-(aq); E0 = -0.83 V
Mg2+(aq) + 2e- → Mg(s); E0 = -2.38 V
If all of these substances were available, what galvanic cell could be set up using these substances that would steadily deliver approximately 1.6 V?
a)
F2/F- and O2/H2O
b)
O2/H2O and Fe2+/Fe
c)
O2/H2O and Cu2+/Cu
d)
H2O/H2 and Mg2+/Mg
2.
The cell reaction occurring in a particular button cell was:
Zn(s) + Ag2O(s) + H2O(l) → 2Ag(s)+ Zn(OH)2(s)
This cell delivered 1.50 V. The half-equation for the silver half-cell is:
Ag2O(s)+ H2O(l)+ 2e-→ 2Ag(s)+ 2OH-(aq); E0 = 0.34 V
The standard redox potential for the zinc half-cell must be:
Zn(s) + Ag2O(s) + H2O(l) → 2Ag(s)+ Zn(OH)2(s)
This cell delivered 1.50 V. The half-equation for the silver half-cell is:
Ag2O(s)+ H2O(l)+ 2e-→ 2Ag(s)+ 2OH-(aq); E0 = 0.34 V
The standard redox potential for the zinc half-cell must be:
a)
-1.16 V
b)
+1.16 V
c)
-1.84 V
d)
+1.84 V
3.
What is the key difference between a galvanic cell and a fuel cell?
a)
Galvanic cells deliver direct current; fuel cells deliver alternating current.
b)
Galvanic cells are essentially for energy storage; fuel cells work continuously.
c)
Galvanic cells do not use gases as reactants; fuel cells only use gases.
d)
Galvanic cells are not rechargeable; fuel cells are constantly recharged.
4.
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
5.
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
6.
A fuel cell can be constructed that uses the two half-reactions as shown.
Which one of the following would occur at the negative electrode of the cell as it generates electricity?
Which one of the following would occur at the negative electrode of the cell as it generates electricity?
a)
production of H+
b)
formation of H2O
c)
consumption of CO2
d)
reduction of CH3OH
7.
A fuel cell can be constructed that uses the two half-reactions as shown.
Which one of the following statements about this fuel cell is most likely to be correct?
Which one of the following statements about this fuel cell is most likely to be correct?
a)
An external power supply is used to recharge the cell.
b)
Gaseous products are recycled into the cell to improve efficiency.
c)
Chemical energy is not completely converted into electrical energy.
d)
More H+ ions are produced at the anode than are consumed at the cathode.
8.
Which one of the following state is true for both fuel cells and rechargeable cells?
a)
All reactants are stored within the cell.
b)
Reaction products are continuously removed from the cell.
c)
Electrons pass from the reductant to the anode as electricity is produced.
d)
Electrical energy is converted to chemical energy as the cell is recharged.
9.
What happens to oxygen molecules in a hydrogen-oxygen fuel cell?
a)
They react with electrons to form oxide ions, O2-
b)
They react with hydrogen ions to form hydroxide ions, OH-
c)
They react with hydrogen ions and electrons to form water
10.
What is the main reason why hydrogen is more difficult to store than diesel?
a)
Hydrogen is a gas at room temperature but diesel is a liquid
b)
Hydrogen can be liquefied by cooling it
c)
Hydrogen can be stored under pressure
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