Consider a galvanic (spontaneous) cell based on the following half-reactions. Wr

Question

Consider a galvanic (spontaneous) cell based on the following half-reactions.

Write the overall reaction for the galvanic cell.

Determine the E0cell for the galvanic cell reaction.

Determine the Ecell for the reaction (298 K) when [Au+3] = 4.3 X 10-4 M and [Tl+] = 2.45 M.

Determine the T, in K, at which the cell potential, Ecell, under the concentration conditions stated in part c), would be zero

Consider a galvanic (spontaneous) cell based on the following half-reactions. Au+3 + 3e- + right arrow TI(s) Eo 1/2 = -0.34 V Write the overall reaction for the galvanic cell. Determine the E0cell for the galvanic cell reaction. Determine the Ecell for the reaction (298 K) when [Au+3] = 4.3 X 10-4 M and [Tl+] = 2.45 M. Determine the T, in K, at which the cell potential, Ecell, under the concentration conditions stated in part c), would be zero Right arrow Au E01/2 = 1.50 V Tl+ + e-

Explanation / Answer

(a)

Write the overall reaction for the galvanic cell.

Au+3(aq) + 3Ti (s) = Au(s) + 3Ti+(aq)

(b)

Determine the E0cell for the galvanic cell reaction.

Cathode(Au+3|Au)

Anode(Ti|Ti+)

E0cell=1.5-(-.34)=1.84V

(c)

Determine the Ecell for the reaction (298 K) when [Au+3] = 4.3 X 10-4 M and [Tl+] = 2.45 M.

Here n=3

Nerst equation

Ecell=1.84-0.059/3*log(2.45/4.3*10^-4)=1.77V

(d)

Determine the T, in K, at which the cell potential, Ecell, under the concentration conditions stated in part c), would be zero

Nerst equation Ecell=0 when

E0cell=0.059/3*T/298*log(2.45/4.3*10^-4) =1.77

Or

E0cell=2.303*8.314*T/(3*96500)*log(2.45/4.3*10^-4) =1.77

T=3*96500*1.77/(2.303*8.314*log(2.45/4.3*10^-4)) =7141K

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