What is the cell potential of the following cell at 25 oC? Note Au is a passive electrode
Cu / Cu2+ (0.00630 M) // Cr3+ (0.670 M), Cr2O72- (0.0660), H1+ (1.00 M) / Au
E =
V
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What is the cell potential of the following cell at 25 oC? Note Au is a...
please answer all wueston Question 33 (3 points) (33) For a galvanic cell notation: (-) Ni /Ni2+ (aq) // Au3+ (aq) / Au (+), The electrode potentials: Eº (Ni2+/ Ni) = -0.257 V, E ° (AU3+ / Au ) = 1.498 V. The cell potential Eºcell (a) 1.241 V (b) - 1.755 V O (0) 1.755 V (d) 1.498 Why Question 35 (3 points) (35) For galvanic cell: (-) Cr/ Cr3+ (aq) / Cu2+ (aq) / Cu(+), the correct half...
A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 oC. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. What are the concentrations of Pb2+ and Cu2+ when the cell potential falls to 0.370 V? Cu2+(ag) + Pb(s) → Cu(s) + Pb2+(ag) Hint: [Pb2+] + [Cu2+] = (1.5M + 0.05M) = 1.55 M total Hint: the standard potential of Pb2+ + 2e- → Pb(s) is -0.130 and the standard potential...
need answers for all questions Question 35 (3 points) (35) For galvanic cell: (-) Cr/ Cr3+ (aq) // Cu2+ (aq) / Cu (+), the correct half reactions are 0 (a) Cr3+ (a) Cr3+ + 3e → Crat (-) electrode; Cu+ 2e → Cu2+ at (+) electrode (b) Cr - 3e → Cr3+ at (-) electrode; Cu2+ + 2e → 2 Cu at (+) electrode Occ) cr (c) Cr + 3e → Cr3+ at (-) electrode; Cu2+ - 2e → Cu...
A voltaic cell consists of a Pb/Pb2+ half-cell and a Cu/Cu2+ half-cell at 25 oC. The initial concentrations of Pb2+ and Cu2+ are 0.0500 M and 1.50 M, respectively. What is the initial cell potential? Hint: the standard potential of Pb2+ + 2e- → Pb(s) is -0.130 and the standard potential of Cu2+ + 2e- → Cu(s) is +0.340. Hint #2: Use [Cu2+] as the product and [Pb2+] as the reactant. The equation we are supposed to use is E= Eo-...
If a platinum indicator electrode is used to measure [Cu^22^++] (standard reduction potential of Cu^22^++ is 0.337 V), and [Cu^22^++] = 0.0053 M, what is the cell potential (V) if the reference electrode is SCE and the measurement is taken at 298 K? Indicator Electrode--Quantification (Homework) Homework Unanswered If a platinum indicator electrode is used to measure [Cu2+] (standard reduction potential of Cu +is 0.337 V), and [Cu2+ o.0053 M, what is the cell potential (V) if the reference electrode...
Question 1) What is the value of the equilibrium constant at 25 oC for the reaction between the pair: Pb(s) and Sn2+(aq) to give Sn(s) and Pb2+(aq) Use the reduction potential values for Sn2+(aq) of -0.14 V and for Pb2+(aq) of -0.13 V Question 2) What is the value of ΔGo in kJ at 25 oC for the reaction between the pair: Cr(s) and Cu2+(aq) to give Cu(s) and Cr3+(aq) Use the reduction potentials for Cr3+(aq) is -0.74 V and...
The cell potential of a redox reaction occurring in an electrochemical cell under any set of temperature and concentration conditions can be determined from the standard cell potential of the cell using the Nernst equation where E is the cell potential of the cell, E° is the standard cell potential of the cell, R is the gas constant, T is the temperature in kelvin, n is the moles of electrons transferred in the reaction, and Q is the reaction quotient....
In the following cell, A is a standard Cu2+Cu electrode connected to a standard hydrogen electrode. If the voltmeter reading is +0.34 V, which half-reaction occurs in the left-hand cell compartment? Given: Standard reduction potential of the H1/H2 and Cu2*/Cu couples are 0.00 and +0.34 V, respectively. Holo H2(g) --> 2H+ (aq) + 2e7 2H(aq) + 2e --> H2(g) Cu(s) --> Cu2(aq) + 2e Cu2(aq) + 2e --> Cu(s)
What is the potential of a cell made up of Zn/Zn2+ and Cu/Cu2+ half-cells at 25°C if [Zn²+1 -1.00 Mand (Cu2+] = 0.05 M?
For the following cell what is the cell potential under standard conditions? Zn + Cu2+ → Cu + Zn2+ If Cu2+ + 2e- → Cu E° = 0.34V and Zn2+ + 2e- → Zn E° = -0.76 V