Reference no: EM132953852

1. Write the cell notation for the following cells. Use Pt for any inert electrodes needed.

(a) Cl2 (g) + 2 Cr2+ (aq) → 2 Cr3+ (aq) + 2 Cl- (aq)

(b) 6 Br- (aq) + Cr2O7 2- (aq) + 14 H + (aq) → 2 Cr3+ (aq) + 3 Br2 (l) + 7 H2O (l)

2. Make a sketch of each of the following galvanic cells. Label anode and cathode.

(a) Pb (s) + 2 Ag+ (aq) → Pb2+ (aq) + 2 Ag (s)

(b) 2 ClO2 (g) + 2 I- (aq) → 2 ClO2 - (aq) + I2 (s)

(c) Mn (s)| Mn2+ (aq) ClO2 - (aq)ClO2 (g) Pt (s)

3. Predict if a reaction occurs. Explain your answer.

(a) Br2 is added to 1M NaI

(b) Br2 is added to 1M NaCl

4. Calculate the cell potential for the following galvanic cells.

(a) Zn(s)|Zn2+(aq)(0.0085 M) ||Cr3+(aq)(0.010 M)|Cr(s)

(b) Ni(s)|Ni2+(aq)(0.200 M) ||Fe3+(aq)(0.400 M), Fe2+(aq)(0.010 M)|Pt

5. Calculate the concentration of Al3+ in the following cell.

Al(s)|Al3+ (aq)(? M) ||Fe2+ (aq)(0.020 M)|Fe(s) E = 1.18 V