Calculate the cell potential E°cell of each of the following electrochemical cells at 25C Sn(s) I...
Calculate the cell potential E°cell of each of the following electrochemical cells at 25C
- Sn(s) I Sn2+ (6.5 x 10-3 M) II Ag + (0.110M) I Ag (s)
- Zn (s) I Zn 2+ (0.500M) II Fe3+ (7.2 x 10-6 M), Fe2+ (0.15M) I Pt
- Pt I H2 (1 atm) I HCl (0.00880M) I Cl2 (1 atm) I Pt
-
Write the overall cell reaction and calculate the value of E°cell for the following: Zn I Zn2+ II Fe 3+ , Fe2+ I Pt
Homework Answers
a)
Sn(s)/Sn+2(6.5 x10^-3M)//Ag+(0.110M)/Ag(s)
according to the given cell representation
oxidation reaction at anode Sn(s) ----------------------- Sn+2(aq) + 2e-
reduction reaction at cathode [ Ag+(aq) + e- ----------- Ag(s) ] x 2
----------------------------------------------------------------------------------------
Sn(s) + 2 Ag+(aq) -------------- Sn+2(aq) + 2 Ag(s)
---------------------------------------------------------------------------------------------
E0 of Sn+2/Sn = - 0.14V
E0 of Ag+/Ag = + 0.80V
E0cell = E0 cathode - E0anode
E0cell = 0.80 - ( - 0.14)
E0cell = 0.94V
n=2 e-
Ecell = E0cell - 0.0591/n log[Sn+2]/[Ag+]^2
Ecell = 0.94 - 0.0591/2 log( 6.5 x10^-3 )/(0.110)^2
Ecell = 0.948V
Ecell = 0.95V
b)
Zn(s) /Zn+2(0.500M)// Fe+3(7.2x10^-6M),Fe+2(0.15M)/Pt
according to given cell representation
oxidation reaction at anode Zn(s) ---------------------- Zn+2(aq) + 2e-
reduction reaction at cathode [ Fe+3(aq) + e- ------------- Fe+2(aq) ] x2
---------------------------------------------------------------------------------------
Zn(s) + 2 Fe+3(aq) ---------------- Zn+2(aq) + 2 Fe+2(aq)
------------------------------------------------------------------------------------------
E0 of Zn+2/Zn = - 0.769V
E0 of Fe+3/Fe+2 = + 0.77V
E0cell = E0cathode - E0 an0de
E0cell = 0.77 - ( - 0.769)
E0cell = 1.539V
n= 2e-
Ecell = E0cell - 0.0591/n log[Zn+2] [ Fe+2]^2/[Fe+3]^2
Ecell = 1.539 - 0.0591/2 log(0.500)(0.15)^2/(7.2x10^-6)^2
Ecell = 1.29V
c) Pt/H2(1 atm)/HCl(0.00880M)/Cl2(1atm)/Pt
according to given cell representation
oxidation at anode H2(g) -----------------------2 H+(aq) + 2e-
reduction at cathode Cl2(g) + 2e- ----------------- 2 Cl-(aq)
--------------------------------------------------------
H2(g) + Cl2(g) ------------------ 2 H+(aq) + 2Cl-(aq)
-------------------------------------------------------------------
E0 of H+/H2 = 0.00V
E0 of Cl2/Cl- = 1.36
E0cell = E0cathode - E0 anode
E0cell = 1.36 - 0.00
E0cell = 1.36V
Ecell = E0cell - 0.0591/n log[H+]^2[Cl-]^2/[H2][Cl2]
Ecell = 1.36 - 0.0591/2 log(0.00880)^2( 0.00880)^2/1x1
Ecell = 1.60V
d)
Zn(s)/Zn+2//Fe+3,Fe+2/Pt
oxidation reaction at anode Zn(s) ---------------------- Zn+2(aq) + 2e-
reduction reaction at cathode [ Fe+3(aq) + e- ------------- Fe+2(aq) ] x2
---------------------------------------------------------------------------------------
Zn(s) + 2 Fe+3(aq) ---------------- Zn+2(aq) + 2 Fe+2(aq)
------------------------------------------------------------------------------------------
E0 of Zn+2/Zn = - 0.769V
E0 of Fe+3/Fe+2 = + 0.77V
E0cell = E0cathode - E0 an0de
E0cell = 0.77 - ( - 0.769)
E0cell = 1.539V
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Calculate the cell
potential E°cell of each of the following electrochemical cells at
25C
Sn(s) I...
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