Question

Calculate the cell potential for the galvanic cell in which the reaction Fe ( s ) + Au 3 + ( aq ) − ⇀ ↽ − Fe 3 + ( aq ) + Au ( s ) occurs at 25 ∘ C , given that [ Fe 3 + ] = 0.00150 M and [ Au 3 + ] = 0.797 M .

Answer 1

To calculate the cell potential for the given galvanic cell reaction, you can use the Nernst equation and the standard cell potential. Plug in the concentrations of Fe3+ and Au3+ and calculate the cell potential using the Nernst equation at 25°C.

Step-by-step explanation:

The cell potential for the galvanic cell can be calculated using the Nernst equation, which is given by: Ecell = E°cell - (0.0592/n) * log(Q)

where E°cell is the standard cell potential, n is the number of electrons transferred in the reaction, and Q is the reaction quotient.

In this case, the reaction is: Fe(s) + Au3+(aq) -> Fe3+(aq) + Au(s)

The standard cell potential can be found in Appendix L. Plugging in the concentrations of Fe3+ and Au3+, as well as the standard cell potential, into the Nernst equation will give the cell potential at 25°C.

Answer 2

0.79 V

Step-by-step explanation:

From Nernst equation:

E= E°- 0.0592/n log [red]/[ox]

Number of electrons transferred=3

[Red]=0.797 M .

[Ox]= 0.00150 M

First we obtain E°= 0.80-(-0.04)= 0.84 V

E= 0.84- 0.0592/3 log [0.797]/[0.00150]

E= 0.84-0.05

E= 0.79 V