Electrochemistry - Cell Notation 1. Choose the cell notation that corresponds to

Question

Electrochemistry - Cell Notation

1. Choose the cell notation that corresponds to an electrochemical cell that has the electrode reactions shown.

Cu2+(aq) + 2e- Cu(s)
Ag(s) + Cl-(aq) AgCl(s) + e-

(a) Ag(s), AgCl(s) l Cl-(aq) ll Cu2+(aq) l Cu(s)

(b) Ag(s), AgCl(s), Cl-(aq) ll Cu2+(aq), Cu(s)

(c) Cu(s) l Cu2+(aq) ll AgCl(s) l Cl-(aq) l Ag(s)

(d) Pt(s) l AgCl(s) l Cl-(aq) ll Cu2+(aq) l Pt(s)

2. Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.

Au(s) l AuCl4-(aq), Cl-(aq) ll F2(g) l F-(aq) l Pt(s)

3. Enter the balanced half reaction that takes place at the cathode for the electrochemical cell shown. Be sure to include electrons.

Pt(s), H2(g) l H+(aq) ll H+(aq), SO42-(aq), H2SO3(aq) l Pt(s)

1. Choose the cell notation that corresponds to an electrochemical cell that has the electrode reactions shown.

Cu2+(aq) + 2e- Cu(s)
Ag(s) + Cl-(aq) AgCl(s) + e-

(a) Ag(s), AgCl(s) l Cl-(aq) ll Cu2+(aq) l Cu(s)

(b) Ag(s), AgCl(s), Cl-(aq) ll Cu2+(aq), Cu(s)

(c) Cu(s) l Cu2+(aq) ll AgCl(s) l Cl-(aq) l Ag(s)

(d) Pt(s) l AgCl(s) l Cl-(aq) ll Cu2+(aq) l Pt(s)

2. Enter the balanced chemical equation including states that describes the electrochemical cell that is represented by the cell notation as shown.

Au(s) l AuCl4-(aq), Cl-(aq) ll F2(g) l F-(aq) l Pt(s)

3. Enter the balanced half reaction that takes place at the cathode for the electrochemical cell shown. Be sure to include electrons.

Pt(s), H2(g) l H+(aq) ll H+(aq), SO42-(aq), H2SO3(aq) l Pt(s)

Explanation / Answer

1. (b) Ag(s), AgCl(s), Cl-(aq) ll Cu2+(aq), Cu(s)

2. 2Au(s) + 3F2(g) + 8Cl-(aq) ---> 2AuCl4-(aq) + 2F-(aq)

3. oxidation half reaction :

H2(g)   ------> 2H+(aq) + 2e-

reduction half reaction :

So4^2-(aq) + 2e- + 4H+(aq) ----> H2SO3(aq) + H2O(l)

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