Question

3. Answer ALL parts. (a) A two compartment potentiometric cell is assembled from metallic Aluminium and metallic Copper as the two electrodes. The standard reduction potentials for Cu$^{2+}$ and Al$^{3+}$ are +0.34 V and -1.66 V respectively. The relevant unbalanced Redox equation for the overall cell reaction is: Al(s) + Cu$^{2+}$(aq) ? Cu (s) + Al$^{3+}$(aq) i) Balance the above redox chemical equation. ii) Calculate the standard potential $E_{cell}^{o}$ for the overall cell. iii) Sketch the above electrochemical cell (graphically), labelling all relevant components and chemicals clearly. iv) Ensure you label the anode and cathode in iii) above and include their sign. Also suggest the chemical composition (possible salts?) of all the solutions present in the cell. v) In your own words and with reference to your sketch in iii) above, explain the relevant processes that allow the above electrochemical cell to produce electricity. vi) Use shorthand notation to describe this cell. vii) Show and explain, using a relevant calculation, whether the above electrochemical cell is galvanic or electrolytic. Clue: The Gibbs free energy of the cell points to the answer. [15 marks]

          3.
Answer ALL parts.
(a)
A two compartment potentiometric cell is assembled from metallic
Aluminium and metallic Copper as the two electrodes. The standard reduction
potentials for Cu$^{2+}$ and Al$^{3+}$ are +0.34 V and -1.66 V respectively. The
relevant unbalanced Redox equation for the overall cell reaction is:
Al(s) + Cu$^{2+}$(aq) ? Cu (s) + Al$^{3+}$(aq)
i)
Balance the above redox chemical equation.
ii)
Calculate the standard potential $E_{cell}^{o}$ for the overall cell.
iii) Sketch the above electrochemical cell (graphically), labelling all
relevant components and chemicals clearly.
iv) Ensure you label the anode and cathode in iii) above and include their
sign. Also suggest the chemical composition (possible salts?) of all the
solutions present in the cell.
v)
In your own words and with reference to your sketch in iii) above,
explain the relevant processes that allow the above electrochemical cell
to produce electricity.
vi)
Use shorthand notation to describe this cell.
vii)
Show and explain, using a relevant calculation, whether the above
electrochemical cell is galvanic or electrolytic. Clue: The Gibbs free
energy of the cell points to the answer.
[15 marks]

3.
Answer ALL parts.
(a)
A two compartment potentiometric cell is assembled from metallic
Aluminium and metallic Copper as the two electrodes. The standard reduction
potentials for Cu^2+ and Al^3+ are +0.34 V and -1.66 V respectively. The
relevant unbalanced Redox equation for the overall cell reaction is:
Al(s) + Cu^2+(aq) ? Cu (s) + Al^3+(aq)
i)
Balance the above redox chemical equation.
ii)
Calculate the standard potential Ecell^o for the overall cell.
iii) Sketch the above electrochemical cell (graphically), labelling all
relevant components and chemicals clearly.
iv) Ensure you label the anode and cathode in iii) above and include their
sign. Also suggest the chemical composition (possible salts?) of all the
solutions present in the cell.
v)
In your own words and with reference to your sketch in iii) above,
explain the relevant processes that allow the above electrochemical cell
to produce electricity.
vi)
Use shorthand notation to describe this cell.
vii)
Show and explain, using a relevant calculation, whether the above
electrochemical cell is galvanic or electrolytic. Clue: The Gibbs free
energy of the cell points to the answer.
[15 marks]

Added by Barbara G.

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