One-half of an electrochemical cell consists of a pure nickel electrode in a solution ofNi2+ ions; the other half is a cadmium electrode immersed in a Cd2+ solution. Usethe following standard emf series Table (if required).Standard ElectrodeElectrode ReactionPotential, V" (V)Au³+ + 3e → Au+1.420O2 + 4H+ + 4ePr2+ + 2e2H2O+1.229Pt-+1.2Ag+ + eFe+ + e→ AgFe2++0.800+0.771Increasingly inert(cathodic)O2 + 2H,O + 4eCu²+ + 2e4(OH)+0.401Cu+0.3402H* + 2ePb2+ + 2eH20.000Pb-0.126Sn2+ + 2eSn-0.136Ni2+ + 2eNi-0.250Co2+ + 2eCd²+ + 2eFe+ + 2eCo-0.277Cd-0.403Fe-0.440Cr+ + 3eCr-0.744Increasingly active(anodic)Zn2+ + 2e¯Zn-0.763AF+ + 3eAl-1.662Mg²+ + 2eMg-2.363Na+ + e –→ Na-2.714K* + e -→ K-2.924If the cell is a standard one, write the spontaneous overall reaction and calculate thevoltage that is generated.Ni2+ + Cd ---> Ni + Cd2+ and +0.153 VNi + Cd2+ ---> Ni2+ + Cd and +0.153 VNi2+ + Cd ---> Ni + Cd2+ and -0.153 VNi + Cd2+Ni2+ + Cd and -0.073 V--->

Since standard reduction potential of Ni+2 is more as compared to Cd+2 so Ni electrode act as…

If the cell is a standard one, write the spontaneous overall reaction and calculate the voltage that is generated. Ni2+ + Cd ---> Ni + Cd2+ and +0.153 V Ni + Cd2+ Ni2+ + Cd and +0.153 V Ni2+ + Cd ---> Ni + Cd2+ and -0.153 V Ni + Cd2+ --> Ni2+ + Cd and -0.073 V

If the cell is a standard one, write the spontaneous overall reaction and calculate the voltage that is generated. Ni2+ + Cd ---> Ni + Cd2+ and +0.153 V Ni + Cd2+ Ni2+ + Cd and +0.153 V Ni2+ + Cd ---> Ni + Cd2+ and -0.153 V Ni + Cd2+ --> Ni2+ + Cd and -0.073 V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

One-half of an electrochemical cell consists of a pure nickel electrode in a solution of
Ni2+ ions; the other half is a cadmium electrode immersed in a Cd2+ solution. Use
the following standard emf series Table (if required).
Standard Electrode
Electrode Reaction
Potential, V" (V)
Au³+ + 3e → Au
+1.420
O2 + 4H+ + 4e
Pr2+ + 2e
2H2O
+1.229
Pt
-+1.2
Ag+ + e
Fe+ + e
→ Ag
Fe2+
+0.800
+0.771
Increasingly inert
(cathodic)
O2 + 2H,O + 4e
Cu²+ + 2e
4(OH)
+0.401
Cu
+0.340
2H* + 2e
Pb2+ + 2e
H2
0.000
Pb
-0.126
Sn2+ + 2e
Sn
-0.136
Ni2+ + 2e
Ni
-0.250
Co2+ + 2e
Cd²+ + 2e
Fe+ + 2e
Co
-0.277
Cd
-0.403
Fe
-0.440
Cr+ + 3e
Cr
-0.744
Increasingly active
(anodic)
Zn2+ + 2e¯
Zn
-0.763
AF+ + 3e
Al
-1.662
Mg²+ + 2e
Mg
-2.363
Na+ + e –→ Na
-2.714
K* + e -→ K
-2.924
If the cell is a standard one, write the spontaneous overall reaction and calculate the
voltage that is generated.
Ni2+ + Cd ---> Ni + Cd2+ and +0.153 V
Ni + Cd2+ ---> Ni2+ + Cd and +0.153 V
Ni2+ + Cd ---> Ni + Cd2+ and -0.153 V
Ni + Cd2+
Ni2+ + Cd and -0.073 V
--->

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