20. Calculate the cell potential for the following cell and indicate whether the reaction is spontaneous: Cu2+ + Pb -> Cu + Pb2+, if [Cu2+ ] = 0.52M and [Pb2* ] = 0.3M Eº Pb2+/Pb = -0.13 V, Eº cu2+/Cu = +0.34 V %D %3D %3D

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.793 M and…

A: The reaction given is Cr (s) + Ni2+ (aq) ↽−−⇀  Cr2+ (aq) + Ni (s) In the above reaction, the…

Q: Use the standard reduction potentials at 25° C in Table 18.1 in Tro, Fridgen and Shaw, and calculate…

A:

Q: For this reaction, Cr20-2 + 14H+ +6l > 2Cr2+ + 312 + 7H20 E°cell = 0.79V AG° 0 and K0 and K>1 AG° 1

A:

Q: A galvanic cell is made of a Ni2+/Ni half cell with [Ni2+] = 1.00 × 10–3 M and a Ag+/Ag half cell…

A:

Q: A galvanic cell is based on the following half reactions: Ag* + e > Ag (s) E° = 0.80 V Cu2+ + 2 e →…

A: The cell potential at a given temperature can be obtained by the following relation: E=E0-RTnFlnK…

Q: Calculate the cell potential for the reaction as written at 25.00 "C, given that [Zn²+] = 0.795 M…

A: Given - [Zn2+] = 0.795 M             [Ni2+] = 0.0180 M             Temperature = 25.00°C

Q: A galvanic cell is made of a Ni²*/Ni half cell with [Ni2*] = 1.00 × 10-3 M and a Ag*/Ag half cell…

A:

Q: Consider the cell: Cd(s) | Cd2 (aq) (0.035M) || Cu2*(aq) (x M)| Cu(s) Cd2+ + 2e → Cd E° = -0.40 V…

A:

Q: At 25 oC a zinc-copper battery is constructed as follows:  Zn|Zn2+(0.1000 M)||Cu2+(2.500 M)|Cu…

A: Using Nerst equation  Ecell  = Eocell - (0.0591/n ) log [ Zn2+ ]/[ Cu2+ ]

Q: Consider the cell: Cd(s) | Cd2*(aq) (0.035M) || Cu2 (aq) (x M)| Cu(s) Cd2* + 2e Cd E° = -0.40 V Cu2*…

A: The half-cell reactions are : Cd2+  +  2e-  →  Cd                E°=-0.40 VCu2+  +  2e-  →  Cu…

Q: Given: Cell Notation       Eocell VO2+/VO2+          1.000 VO2+/V2+            0.360 VO2+/V3+…

A: Latimer diagram: It is data of the standard electrode potential of the chemical element that is…

Q: Cd(s)| Cd2 (aq) (0.035M) || Cu2"(aq) (x M Cu(s) Cd2* + 2e → Cd E = -0.40 V Cu2* + 2e → Cu E = +0.34V…

A:

Q: Calculate the cell potential for this reaction, in the direction shown, at 298 K. Ni?+ (1.05 M) Ni2+…

A: Given reaction: Ni2+1.05 M→Ni2+9.10×10-5 M Temperature = 298 K

Q: The above cell shows the standard half-cell potentials as follows: Put +e 4+ + Pu3+ E° = 0.97V…

A: Oxidation half reaction: Pu4+ + e = Pu3+         E0 (Ox) = 0.97 V Reduction half reaction: Cr2O72- +…

Q: Given the following cell at 25°C: CuļCuso4 (0.0200 M) || Fe2* (0.0200 M), Fe3* (0.0100 M), HCI (1.00…

A:

Q: It is desired to separate silver in a solution that is 0.0481 M BiO*, 0.119 M Cu2+, 0.0916 M Ag*,…

A:

Q: Calculate the emf of the following cell at 298 K: Al(s)/Al3+ (0.15M)//Cu2+ (0.025M) /Cu(s) Given Eo…

A: Welcome to bartleby !  Introduction :  We have to calculate Ecell of the reaction .

Q: Consider the cell: Cd(s) | Cd2 (aq) (0.035M) || Cu2 (aq) (x M)| Cu(s) Cd2* + 2e → Cd E° = -0.40 V…

A: The concentration of Cu2+ is given below

Q: Consider the cell: Cd(s) | Cd2+(aq) (0.035M) || Cu2+(aq) (x M)| Cu(s) Cd2+ + 2e → Cd E° = -0.40 V…

A: In this given question we want to calculate the concentration Cu2+ so we can use the Nernst equation…

Q: Consider the cell: Cd(s) | Cd2*(aq) (0.035M) || Cu²*(aq) (x M)| Cu(s) Cd2+ + 2e Cd E° = -0.40 V Cu2+…

A: Given Conditions for Question 1 [Cd+2] = 0.035 M Ecell = 0.77 V R = 8.314J/mol.K F = 96485J/mol.V…

Q: Calculate the cell potential, ∆G, and equilibrium constant for the reaction Ca(s) + Mn2+(aq) (1M) ⇌…

A:

Q: cell employs the redox reaction: 2 Fe 3*caq) + 3 Mqis) 2 Fecs) +3Mg"caqı Calaulate he cell potential…

A: The given chemical reaction is: 2Fe3+(aq)+3Mg(s) → 2Fe(s)+3Mg2+(aq) The given information is: Conc.…

Q: A galvanic cell consists of a Cr+/Cr half-cell with unknown [Cr³+] and a Ni²+/Ni half-cell with…

A: GALVANIC CELL: It is a type of an electrochemical cell which is utilized to provide electricity by…

Q: %3D Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.884…

A: In an electrochemical cell, there are two compartments, the one in which oxidation reaction takes…

Q: Calculate the cell potential for the following concentration cell at 25 °C.…

A: Here the cell represented consists of a cathode and the anode made up of nickel. In the cell…

Q: A galvanic cell is made of a Ni*/Ni half cell with [Ni²-] = 1.00 × 103 M and a Ag:/Ag half cell with…

A: We can solve the problem by constructing the cell first. We can write the two half reactions to…

Q: 19.85 Calculate the cell potential of the following cell at 25°C. Cr(s) Cr **(1.0 x 10 ³ M) | |…

A:

Q: Write electrode reaction, cell reaction and calculate the EMF of the following cell at 25°C. Fe | Fe…

A: Nernst equation is, E=E0cell-RTnF×lnQ T= temperature in Kelvin. n = number of electrons involved. F…

Q: The standard electrode potential for the reduction of Ni²+ to Ni is – 0.25 V. Would the potential of…

A:

Q: Given that standard reduction potentials at 298.15 K are E° Ag+ /Ag = +0.800 V and E° Cu?"/Cu =…

A: When Ag foil is soaked into Cu(NO3)2 solution, for Ag to dissolve the reaction involved would be:…

Q: is desired to separate silver in a solution that is 0.0613 M 0.0955 Ag', and 0.500 by…

A: Applying the Nernst equation, the cell potential at 298 K (25 °C) is, Ecell = E0cell -0.0592VnlogQ

Q: An electrochemical cell consists of a nickel metal electrode immersed in a solution with [Ni2+] =…

A: Given : Concentration of Ni2+, [Ni2+ ] = 1.0 M Concentration of OH-, [OH- ] = 1.0 X 10-4 M And cell…

Q: The following redox reaction was performed under non-standard conditions. Zn(s) + Cu2+(aq) →…

A: Given, Concentration of Zn2+ = 0.113 M Concentration of Cu2+ = 1.08 M Data from General data,…

Q: A concentration cell is constructed by placing identical Cu electrodes in two Cu2+ solutions. If the…

A: E◦ for Cu2+ to Cu is 0.342. But concentration cell is formed with same metal. So the E◦cell is 0.

Q: (c) A cell employs the following half-reactions. Ni2+ (aq) + 2e Cr³+ (aq) + 3e Ni(s) Cr(s) E° =…

A:

Q: A galvanic cell is made of a Ni2+/Ni half cell with [Ni2+] = 1.00 x 10-3 M and a Ag*/Ag half cell…

A: This is the concept of electrochemistry

Q: A solution containing Pt+ is electrolyzed with a current of 2.60 A. How long will it take to plate…

A:

Q: 13.28 For the cell Pt,|Fe²*(a = 2.00), Fe**(a = 1.20); I"(a = 0.100)|1,(s)|Ptg %3D (a) write the…

A:

Q: 3. Calculate the voltage of a cell composed of Ni2+|Ni and Cu2+ | Cu electrodes at 298 K, if ANi 2+…

A: Here we will use the Nernst equation to find the voltage. Ecell = E0 - (RT/nF)ln Q where Q =…

Q: The following cell potentials have been measured for Cu/Cu2+ (1.0, 0.1, 0.01, 0.001, and 0.0001 m)…

A: The concentrations of the CuSO4 solutions are 0.0001 m, 0.001 m, 0.01 m, 0.1 m, 1 m The ionic…

Q: Given the following cell at 25°C: CuļCuso4 (0.0200 M) || Fe2* (0.0200 M), Fe3* (0.0100 M), HCl (1.00…

A: The electrode potential of a cell represented as  Cu|CuSO4(0.0200 M) || Fe2+(0.0200 M), Fe3+(0.0100…

Q: The standard reduction potentials are-0.13 V for Pb2+ and +0.80 V for Ag+. Calculate E'cell for the…

A: E°Cell = E°red - E°oxi Lower reduction potential values always undergo oxidation  Higher reduction…

Q: Calculate the cell potential of the following cell at 25°C. Cr(s)|Cr³*(1.0 × 10-3 M)||Ni²*(1.5…

A: The half-cell reaction involved in the given cell and the standard reduction potential is given…

Q: If E° cell for the couples Fe 3+ /Fe 2+ ; MnO 4 2- ,H+ /Mn 2+ /v 2+ and Br 2 /Br are +0.77, +1.51,…

A: Given, E° cell for the couples Fe2-/Fe3+ ; MnO42-,H+/Mn2+,H2O ; Zn2+/Zn ; V3+/V2+ ; Br2/Br-  +0.77,…

Q: A galvanic cell is made of a Ni2+/Ni half cell with [Ni²+] = 1.00 × 10-3 M and a Ag*/Ag half cell…

A:

Q: 30. Calculate the emf of the following cell at 298 K: Al(s)/Al3+ (0.15M)//Cu2 (0.025M) /Cu(s) (Given…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.876 M and…

A: Given reaction is :  Cr (s) +  Ni2+ (aq) ↽−−⇀ Cr2+ (aq) + Ni (s) Calculate the cell potential for…

Q: For the cell diagram: Mg(s)|Mg2+(aq)|2H+(aq)|H2(g)|Pt(s) which reaction occurs at the anode?

A:

Q: he cell described below: Zn|Zn2+(1.00 M)||Cu²+(1.00 M)|Cu che cell potential after the reaction has…

A: The given cell is, Therefore,