Question

Use the reduction potentials, the unbalanced half reactions and the unbalanced chemical equation below to answer the following questions:

Reaction	E° (V)
In+(aq) + e− → In(s)	-0.140
In3+(aq) + e− → In(s)	-0.338

In(s) + In³⁺(aq) → In⁺(aq) + In(s)

1. Determine E_cell (in V) for this reaction in the direction shown. Report your answer to three decimal places in standard notation (i.e. 1.234 V).

Tries 0/5

2. Determine ΔG° (in kJ) for this reaction. Report your answer to three significant figures in scientific notation (i.e. 1.23e4 kJ).

Answer 1

1)

Oxidation cell is In+/In which occur at anode

So,

Eo anode = -0.140 V

Reduction cell is In3+/In which occur at cathode

So,

Eo cathode = -0.338 V

Now use:

Eo cell = Eo cathode - Eo anode

= -0.338 V - (-0.140 V)

= -0.198 V

Answer: -0.198 V

2)

Balanced reaction is:

3 In(s) + In3+(aq) —> 3 In+(aq) + In(s)

number of electrons being transferred, n = 3

F = 96500 C

use:

ΔG = -n*F*E

= -3*96500.0*-0.198

= 57321 J

= 57.3 KJ

Answer: 5.73e1 KJ