1. Write out the half reactions, the net chemical reaction and the Eo for the following electrochemical cell: 2+ 2. Write out the half reactions, the net chemical reaction and the E for the following electrochemical cell: Zn (s)| Zn2 (aq), 0.10 M Il Ag (aq), 2.5 M IAg (s) 3. Describe how you would make 45 mL of a 0.10 M tin(II) chloride solution using a common soluble salt. 149 Solution Answer: (1) Given electrochemixal cell is Al(s)/Al^+3(aq), 1.0 M//Sn^+2(aq), 1.0M/Sn(s) Oxidation half cell (at Anode) Al(s) ------> Al^+3(aq) + 3e^- E°(Al^+3/Al)=-1.66 V, Reduction half cell (at cathode) Sn^+2(aq) + 2e^- --------> Sn(s) . E°(Sn^+2/Sn)=-0.14. After balancing, 2Al(s) -------> 2Al^+3(aq) + 6e^- 3Sn^+2(aq) + 6e^- -----> 3Sn(s) -------------------------------------------------- 2Al(s) + 3Sn^+2(aq) --------> 2Al^+3(aq) + 3Sn(s) Net chemical reaction. E°cell=E°cathode - E°anode E°cell=(-0.14 V) - (-1.66 V) E°cell=1.52 V. As per our guidelines I answered first question. Thank you. .

1. 1. Write out the half reactions, the net chemical reaction and the Eo for the following
electrochemical cell: 2+ 2. Write out the half reactions, the net chemical reaction and the E for
the following electrochemical cell: Zn (s)| Zn2 (aq), 0.10 M Il Ag (aq), 2.5 M IAg (s) 3. Describe
how you would make 45 mL of a 0.10 M tin(II) chloride solution using a common soluble salt.
149
Solution
Answer:
(1) Given electrochemixal cell is
Al(s)/Al^+3(aq), 1.0 M//Sn^+2(aq), 1.0M/Sn(s)
Oxidation half cell (at Anode)
Al(s) ------> Al^+3(aq) + 3e^- E°(Al^+3/Al)=-1.66 V,
Reduction half cell (at cathode)
Sn^+2(aq) + 2e^- --------> Sn(s) . E°(Sn^+2/Sn)=-0.14.
After balancing,
2Al(s) -------> 2Al^+3(aq) + 6e^-
3Sn^+2(aq) + 6e^- -----> 3Sn(s)
--------------------------------------------------
2Al(s) + 3Sn^+2(aq) --------> 2Al^+3(aq) + 3Sn(s) Net chemical reaction.
E°cell=E°cathode - E°anode
E°cell=(-0.14 V) - (-1.66 V)

2. E°cell=1.52 V.
As per our guidelines I answered first question. Thank you.