i) Consider an electrochemical cell involving Zinc and Chromium. Zn2+, (aq) + 2e- Zn(s) E° = -0.76 V %3D Cr3+ (aq) + Зе- Cr(s) E° = -0.74 V %3D a) What is the standard reduction potential of anode? b) What is the standard reduction potential of cathode? c) Calculate the potential of this cell under standard conditions(E°cell).

Q: Electrochemistry. Consider the redoxreaction, for which E 8. Co S 1.10 v. Zn(s) Cuaq) - Zn (aq)…

A: Oxidation state or oxidation number of an atom refers to the charge on that atom that it would have…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777…

A: Given-> 2H+(aq) + 2e- ------> H2(g) E°= 0.00 V Cd2+(aq) + 2e- -------> Cd(s)  E°= -0.403 V…

Q: Calculate the Eell for the cell reaction at 25 °C. Take note, not E°.el- 3 Zn (s) + 2 Cr²+ (aq) 3…

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Q: A current of 10.0 amperes flows for 2.00 hours through an electrolytic cell containing a molten salt…

A: According to the reaction given, we have  Xn+ (aq) + ne-→X (s) t=2 hours=7200 sec (since 1 hr =3600…

Q: Calculate E°cell. Mn(s) + Fe2+(s) (aq) ↔ Mn2+ (aq) + Fe (s) a)E°cell =  ?V  b) Calculate E° for…

A: a) Eocell = Eored cathode - Eored anode  Here cathode: Fe2+ (aq) / Fe (s) Therefore, Eored cathode =…

Q: l'or the cell shown, the measured cell potential, Eell, is -0.3657 V at 25 °C. Pt(s) | H, (g, 0.717…

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Q: A concentration cell based on the following half reaction at 288 K Ag +e Ag; SRP = 0.80V is made…

A: Reaction on L.H.E.: Ag(s) ⇌Ag+(0.354M) + e- A⏜A (oxidation) Reaction on R.H.E. Ag+(1.4 M)+e-⇌Ag(s)…

Q: 5. If you constructed a galvanic cell using an electrode X+IX connected to a standard copper…

A: In the cell or galvanic cell , if two  standard half-cell electrode are connected then the resultant…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

A:

Q: The standard reduction potential for Zn2+ is -0.76 V. Calculate the voltage of the following cell at…

A: The reaction at anode i.e oxidation, Zn(s)------------>Zn2+(aq)+2e-........................E0=…

Q: Using table of standard reduction potentials, find the ksp of Hg2Br2.   1)Write the balanced…

A: a) The balanced half cell reactions are as follows:' Anode (oxidation)       2Hg(l)→Hg22+(aq)+2e-…

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

A: Anode half cell reaction: Cathode Half reaction: Overall reaction taking place is as follows:

Q: For the Zn–Cu voltaic cell shown in Figure , we haveZn(s) + Cu2+(aq, 1 M2)----->Zn2+(aq), 1 M) +…

A: Redox reaction- the reaction in which oxidation and reduction takes place simultaneously called as…

Q: current of 15.0 A is passed through a solution of CrCl2 for 45 min. (a) How many grams Cr is…

A: When current is passed through an aqueous solution of CrCl2 , it gets electrolyzed resulting in the…

Q: The free energy change for the following reaction at 25 °C, when [Cr³+] = 7.70x10-3 M and [Cu2+] =…

A:

Q: Ni+ (ag) + Cd(s) → Ni(s) + Cd?+ (aq) E cell = +0.15 V Under standard conditions, a Ni-Cd galvanic…

A: A Galvanic cell is made up of an anode and a cathode.   Reduction reaction occurs at cathode whereas…

Q: The following reaction proceeds spontaneously under standard conditions because E°cell > 0 (which…

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Q: A cell is set up with copper and lead electrodes in contact with CUSO4(aq) and Pb(NO3)2(aq),…

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Q: The standard oxidation potential of Ni/Ni2+ electrode is 0.3 V. If this is combined with a hydrogen…

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Q: A cell is prepared by dipping a copper rod in 0.01 M CuSO4 solution and zinc rod in 0.02 M of ZnSO4…

A: Given :  E°Zn+2/Zn  = -0.76 V  E°Cu+2/Cu = 0.34 V  [CuSO4] = 0.01 M  [ZnSO4] = 0.02 M

Q: A voltaic cell is made by placing an iron electrode in a compartment in which the Fe2+concentration…

A: The half reactions of the galvanic cell are:Fe (s) → Fe2+ (aq) + 2 e-2 H+ (aq) + 2 e- → H2 (g) The…

Q: Consider Zn+2 (0.056 M) | Zn || TI*3 (9.86 x 102M) I TI* (0.048 M) Pt E° (Zn*2/ Zn) = -0.763 V E°…

A: On the left half of the cell representation there is anode and on the right it is the cathode. Ecell…

Q: A galvanic cell is made from two half-cells. In the first, a platinum electrodeis immersed in a…

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Q: In some applications nickel–cadmium batteries have beenreplaced by nickel–zinc batteries. The…

A:

Q: The following galvanic cell has 8° = +1.887 V at 25°C: Co(s) | Co2+ (aq) || Ce4+ (aq), Ce3+ (aq) |…

A: The solution is as follows:

Q: Half-Reaction Standard Reduction Potential, E (V) Ag* (aq) +e- -→ Ag(s) +0.80 Cu?+ (aq) + 2 e- →…

A: The correct option is explained below.

Q: John makes a galvanic cell with the half reactions Mt3+(aq) + 3e1- -->Mt(s), and R2+(aq) + 2e1- -->…

A: Given that Standard reduction potentials of cathode and anode  1.09 V and 0.34 V respectively.…

Q: Calculate AGexn and K for each of the following reactions. Part C The disproportionation of MnO2 (s)…

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Q: A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at…

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Q: i) Consider an electrochemical cell involving Nickel and Copper. Ni2* (a0) + 2e- → Nis E° = -0.25 V…

A: On the basis of Reduction potential, the substances which have the lower reduction potentials are…

Q: Using tne following half- cell values from the two equations Fe*(aq) + 2e Fe(s); Eo =-0.44 V Cu*(aq)…

A:

Q: Consider an electrochemical cell based on the following cell diagram ven that the standerd cell emf…

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Q: For the cell shown, the measured cell potential, Ecet, is -0.3715 V at 25 °C. P(s) | H,(g.0.857 atm)…

A: Given- Ecell =-0.3715V  PH2=0.857atm Concentration of Cd2+=1.00M

Q: You wish to construct an electrochemical cell from the following half- reactions: Ag* (ag) + e -->…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Consider the following galvanic cell and calculate the cell potential (Ecell). Co(s) | Co2"(aq, 0.15…

A:

Q: For the cell shown, the measured cell potential, Ecell, is -0.3521 V at 25 °C. Pt(s) | H,(g, 0.785…

A:

Q: If the concentration of Ag* is 0.0115 M, the concentration of H* is 0.355 M, and the pressure of H2…

A: Use Nernst equation, to get the cell potential:

Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

A:

Q: A hydrogen electrode is immersed in a 2.0M solution of acetic acid at 25 °C. This electrode is…

A:

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag     ℰ° = +0.80 V…

A: The cell's feasibility as well as potential are estimated using Nernst equation which derives the…

Q: For the cell shown, the measured cell potential, Ecel, is-0.3621 V at 25 °C. Pt(s) | H, (g,0.853…

A:

Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

A: The process in which a metal coating is applied on another piece of metal using an…

Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

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Q: 1) For the following combination of electrodes and solutions, indicate, 0.340 V a) Anode, cathode…

A: E° Cu2+/Cu is 0.34 V E° Ag+/Ag is 0.79 V Ag+ gets reduced and Cu gets Oxidised.

Q: For the galvanic (voltaic) cell Fe(s) + Mn2" (aq) Fe2*(aq) + Mn(s) (E° = 0.77 V at 25°C), what is…

A: We can use the Nernst equation to calculate the Ecell of a reaction. We have to get number of…

Q: A voltaic cell is constructed using an Cr metal electrode in a 1.00 M Cr3+ solution, and the other…

A: Cr3+  +  3e-⟶ Cr(s)  Eo = -0.740 V Ni2+  +  2e-⟶ Ni(s)  Eo = -0.250 V

Q: A hydrogen electrode is immersed in a 1.9 M solution of acetic acid at 25 "C. This electrode is…

A:

Q: Zebulon needs to measure the unknown concentration of Sn2+. A Galvanic cell is set up in a room with…

A: This question is solve by using nernest equation . In this question we have to find out the…

Q: Calculate £º, E, and AG for the following cell reaction: 3+ 3Zn(s) + 2Cr³+ (aq) = 3Zn²+ (aq) + 2 Cr…

A: Given-> [Cr3+] = 0.090 M [Zn2+] = 0.0055 M 3Zn(s) + 2Cr3+(aq) <-----> 3Zn2+(aq) + 2Cr(s)