contestada

An electrochemical cell is based on the following two half-reactions:
Ox: Sn(s)→Sn2+(aq, 1.85 M )+2e−
Red: ClO2(g, 0.150 atm )+e−→ClO−2(aq, 2.00 M )

Compute the cell potential at 25 ∘C.
Ecell =_______V
Dont answer this if you dont know the answer please this is a matter of a passing grade in a class.

Respuesta :

Ecell=E°cell-(RT/nF)lnQ 
E°cell=1.09V 
R=8.314 
T=298K 
n=2 (2 electrons are passed from Sn2+ to 2ClO) 
F=96485 
Q=8.32 (2.00/0.100*1.55^2) Therefore; 
1.09-(8.314*298/2*96485)ln8.32 
1.09-(0.0128)ln8.32 
1.09-(0.0128)2.12 
1.09-0.027=1.06V 
pstnonsonjoku

Given the available information in the question, the cell voltage is 0.98 V.

The overall equation of the reaction is; Sn(s) + 2ClO2(g) -----> Sn2+(aq) + 2ClO2−(aq)

From the question, we know that;

[Sn2+] = 1.85 M

[ClO2−] = 2.00 M

[ClO2] = 0.150 atm

n = 2 electrons

The standard cell potential is obtained from;

E°cathode = 0.93 V

E°anode = -0.13 V

E°cell = 0.93 V - ( -0.13 V) = 1.06 V

Using Nernst equation;

Ecell = E°cell - 0.0592/2 log Q

Q = [Sn2+] [ClO2−]^2/[ClO2]^2

Q = [ 1.85] [2.00]^2/[0.150]^2

Q = 328.89

Ecell =  1.06 - 0.0592/2 log( 328.89)

Ecell = 0.98 V

Learn more: https://brainly.com/question/6505878

Otras preguntas