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, Vº (V) Au3+ + 3e- → Au +1.420 O2 + 4H* + 4e Pr2+ + 2e – Pt 2H2O +1.229 - +1.2 Ag* + e – Ag Fe2+ +0.800 Fet + e +0.771 Increasingly inert (cathodic) O2 + 2H,O + 4e¯ → 4(OH¯) Cu²+ + 2e¯ +0.401 Cu +0.340 2H* + 2e – H2 Pb2+ + 2e 0.000 Pb -0.126 Sn2+ + 2e Sn -0.136 Ni2+ + 2e – Ni -0.250 Co2+ + 2e – → Co -0.277 Cd2+ + 2e → Cd -0.403 Fe2+ + 2e Fe -0.440 Cr+ + 3e - → Cr -0.744 Increasingly active (anodic) Zn2+ + 2e → Zn -0.763 A+ + 3e Al -1.662 Mg+ + 2e Mg -2.363 Nat + e - Na -2.714 K* + e - K -2.924 Calculate the cell potential at 25°C if the Cd2+ and Ni2+ concentrations are 0.5 and 10-3 M, respectively, and write the spontaneous overall reaction in this situation. -0.153 V and Ni + Cd2+ ---> Ni2+ + Cd +0.073 V and Ni + Cd2+ Ni2+ + Cd ---> +0.073 V and Ni2+ + Cd ---> Ni + Cd2+ -0.073 V and Ni²+ + Cd ---> Ni + Cd2+

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, Vº (V) Au3+ + 3e- → Au +1.420 O2 + 4H* + 4e Pr2+ + 2e – Pt 2H2O +1.229 - +1.2 Ag* + e – Ag Fe2+ +0.800 Fet + e +0.771 Increasingly inert (cathodic) O2 + 2H,O + 4e¯ → 4(OH¯) Cu²+ + 2e¯ +0.401 Cu +0.340 2H* + 2e – H2 Pb2+ + 2e 0.000 Pb -0.126 Sn2+ + 2e Sn -0.136 Ni2+ + 2e – Ni -0.250 Co2+ + 2e – → Co -0.277 Cd2+ + 2e → Cd -0.403 Fe2+ + 2e Fe -0.440 Cr+ + 3e - → Cr -0.744 Increasingly active (anodic) Zn2+ + 2e → Zn -0.763 A+ + 3e Al -1.662 Mg+ + 2e Mg -2.363 Nat + e - Na -2.714 K* + e - K -2.924 Calculate the cell potential at 25°C if the Cd2+ and Ni2+ concentrations are 0.5 and 10-3 M, respectively, and write the spontaneous overall reaction in this situation. -0.153 V and Ni + Cd2+ ---> Ni2+ + Cd +0.073 V and Ni + Cd2+ Ni2+ + Cd ---> +0.073 V and Ni2+ + Cd ---> Ni + Cd2+ -0.073 V and Ni²+ + Cd ---> Ni + Cd2+

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 – Pt
2H2O
+1.229
- +1.2
Ag* + e –
Ag
Fe2+
+0.800
Fet + e
+0.771
Increasingly inert
(cathodic)
O2 + 2H,O + 4e¯ → 4(OH¯)
Cu²+ + 2e¯
+0.401
Cu
+0.340
2H* + 2e – H2
Pb2+ + 2e
0.000
Pb
-0.126
Sn2+ + 2e
Sn
-0.136
Ni2+ + 2e – Ni
-0.250
Co2+ + 2e – → Co
-0.277
Cd2+ + 2e → Cd
-0.403
Fe2+ + 2e
Fe
-0.440
Cr+ + 3e - → Cr
-0.744
Increasingly active
(anodic)
Zn2+ + 2e → Zn
-0.763
A+ + 3e
Al
-1.662
Mg+ + 2e
Mg
-2.363
Nat + e - Na
-2.714
K* + e - K
-2.924
Calculate the cell potential at 25°C if the Cd2+ and Ni2+ concentrations are 0.5 and
10-3 M, respectively, and write the spontaneous overall reaction in this situation.
-0.153 V and Ni + Cd2+ ---> Ni2+ + Cd
+0.073 V and Ni + Cd2+
Ni2+ + Cd
--->
+0.073 V and Ni2+ + Cd ---> Ni + Cd2+
-0.073 V and Ni2+ + Cd ---> Ni + Cd2+

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A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr3+ (aq) + 3 Ca(s) → 2Cr(s) + 3Ca²+ (aq) Suppose the cell is prepared with 6.35 M Cr³+ in one half-cell and 0.492 M Ca2+ in the other half. Calculate the cell voltage under these conditions. Cr3+ (aq) + 3e → Cr(s) Ered = -0.744 V Ca2+ (aq) + 2e → Ca(s) Ered = -2.868 V The standard cell potential (E°) for this galvanic cell is [Select] V. There are [ Select] + moles of electrons transferred during to operate this galvanic cell. Under these conditions, the reaction quotient is [Select] and the cell volatage is [Select] V. In order to increase the cell voltage for this cell, [Select ]
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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…
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