[References]What are the overall cell reaction and the cell potential for this voltaic cell?Mg(s)|Mg²+ (ag) || Sn²+ (aq)|Sn(s)Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°CCathode (Reduction)StandardHalf-ReactionPotential, E° (V)Mg²+ (aq) + 2e → Mg(s)-2.38Sn²+ (ag) + 2e → Sn(s)-0.14(Use the lowest possible coefficients. Be sure to to specify states such as (aq) or (s). If a box is not needed, leave it blank.)++E cellVSubmit AnswerTry Another Version10 item attempts remaining A voltaic cell is constructed from a half-cell in which a aluminum rod dips into a solution of aluminum nitrate,Al(NO3)3, and another half-cell in which a lead rod dips into a solution of lead(II) nitrate,Pb(NO3)2. The two half-cells are connected by a salt bridge. Aluminum metal is oxidized during operation of the voltaic cell. What is the half-reaction that occurs at the cathode?(Use the lowest possible coefficients. Be sure to to specify states such as (ag) or (s). If a box is not needed, leave it blank.)+

The electrochemical cell consists of two half-cell reactions where there is oxidation and reductions…

What are the overall cell reaction and the cell potential for this voltaic cell? Mg(s)|Mg* (aq) || Sn²* (aq)|Sn(s) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) Mg+ (aq) + 2e¯ → Mg(s) -2.38 Sn²+ (aq) + 2e¯ → Sn(s) -0.14 (Use the lowest possible coefficients. Be sure to to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Ecell V

What are the overall cell reaction and the cell potential for this voltaic cell? Mg(s)|Mg* (aq) || Sn²* (aq)|Sn(s) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard Half-Reaction Potential, E° (V) Mg+ (aq) + 2e¯ → Mg(s) -2.38 Sn²+ (aq) + 2e¯ → Sn(s) -0.14 (Use the lowest possible coefficients. Be sure to to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Ecell 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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A galvanic cell Mn(s)|Mn2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Mn electrode that weighs 34.9 g and a Pb electrode immersed in 532 mL of 1.00 M Pb2+(ag) solution. A steady current of 0.0519 A is drawn from the cell as the electrons move from the Mn electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? (c) How much mass has the Pb electrode gained when the cell is completely discharged? g (d) What is the concentration of the Pb2+(aq) when the cell is completely discharged? (Assume that the limiting reactant is 100% reacted.) M
For the cell shown, the measured cell potential, Ecell, is -0.3619 V at 25 °C. Pt(s) | H₂(g, 0.721 atm) | H¹ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2 e H₂(g) Eº = 0.00 V Cd²+ (aq) + 2e → Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+] = TOOLS x10 M
Fe (s) +3 Au (aq) ^ + Fe log ^ 3+ +3 Au (s) For the first part, identify the oxidation half-reaction , identify the reduction half- reaction, identify the oxidizing agent, and identify the reducing agent under standard conditions. Next, calculate the standard cell potential, E for the reaction . cell E^ red +1.69 V Half-reaction Au^ + (aq) + e^ - Au (s) Fe^ 3+ (aq) + 3 e^ - Fe (s) -0.040 V Now , calculate the non- standard cell potential , when [Au^ + ]=0.0015 M and the [Fe^ 3+ ]= 0.033 M. After finding the cell potential , calculate the Gibb's free energy , AG Finally, calculate the equilibrium constant , K. Express your answers in two significant digits . Show your work for partial credit . Under non -standard conditions , is this reaction spontaneous or nonspontaneous ? Are reactants or products favored at equilibrium under non -standard conditions ?
Construct a galvanic cell from MnO4- (aq)/MnO2 (s) and H2 O2 (aq)/H2 O (l).a) Write a balanced equation for the cell.b) What is the value of E°cell? standard Ni (s) | Ni2+ (aq) || Ag+ (aq) | Ag (s) is constructed and the standard cell potential is1.03 V.a) Write a balanced reaction for the cell.b) What is ∆G° for the cell?
Consider the following electrochemical cell at 25 C: Pt|H2(g,p)|HCl(aq), 0.010 mol.kg-1|AgCl(s)|Ag For this cell the cell reaction is as follows: 2AgCl(s) + H2(g)  2Ag(s) + 2HCl(aq) (a) Give the electrode half-reactions and determine the standard cell potential.
Consider the following galvanic cell at 25°C. Pt | Cr²+ (0.25 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co The overall reaction and equilibrium constant value are given below. 2 Cr²+ "(aq) + Co2+ Calculate the cell potential & for this galvanic cell and AG for the cell reaction at these conditions. + (aq) → 2 Cr³+ (aq) + Co(s) K = 2.79x107
Consider the same diagram of a galvanic cell as in previous question, conventional current anode X X+ (aq) (C) 0.76 V (D) 0.91 V A e flow Salt bridge Y+ (aq) cathode where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq). Given the following electrode potentials: Ag (aq) + e-> Ag(s); E° = 0.80 V Ni²+ (aq) + 2e --> Ni(s): E = -0.23 V What is the Ecell at 25°C when the electrolyte concentrations are [Ag*] = 1.3 x 10-5 M and [Ni²+] = 0.10 M. (A) 1.15 V (B) 1.30 V
Give the standard line notation for each cell. (a) 2 IO3 (aq) + 10 Fe2+ (ag) + 10 H* (aq) = 10 Fet (ag) + I2 (aq) + 5 H2O(1) O Pt(s) | Fe?+ (aq), Fe+ (ag) || IO3 (ag), Ht (ag), I2 (ag) | Pt(s) O Pt(s) | Fet (aq), I2 (ag) || Fe2+ (ag), IO3 (ag), H* (ag) | Pt(s) Pt(s) | IO3 (ag), H* (ag), I2 (aq) || Fe2+ (ag), Fet (ag) | Pt(s) Pt(s) | Fe2+ (ag), IO3 (ag), H* (aq) || Fet (aq), I2 (ag) | Pt(s) (b) Zn(s) + 2 Ag* (ag) = Zn?+ (aq) + 2 Ag(s) O Zn(s) | Zn?+ (aq) || Ag* (aq) | Ag(s) O Zn(s) | Ag* (aq) || Zn?+ (ag) | Ag(s) Ag(s) | Ag* (ag) || Zn2+ (aq) | Zn(s) O Ag(s) | Zn?+ (aq) || Ag* (aq) | Zn(s) (c) H2O2 (aq) + 2 H* (ag) + 2 e → 2 H2O(1) E = 1.78 V 02 (9) + 2 H* (ag) + 2 e + H2O2 (ag) E = 0.68 V O Pt(s) | O2(9) | H2O2 (aq), H* (ag) || H2O2 (ag), H* (ag) | Pt(s) Pt(s) | H2O2 (aq), H* (ag) || O2 (9) | H2O2 (ag), H* (ag) | Pt(s) Pt(s) | H2O2 (aq) | O2(9) || H* (aq) | Pt(s) O Pt(s) | H2O2(aq) | Pt(s) (d) Mn2+ (aq) + 2 e → Mn(s) E° = - 1.18 V Fe+ (aq) + 3 e → Fe(s) E - -0.036 V O Mn(s) | Mn²+ (ag)…
For the cell shown, the measured cell potential, Ecell, is −0.3627 V at 25 °C. Pt(s) | H2(g,0.735 atm) | H+(aq,? M) || Cd2+(aq,1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, ?o, are 2H+(aq)+2e−⟶H2(g) ?o=0.00 V Cd2+(aq)+2e−⟶Cd(s) ?o=−0.403 V Calculate the H+ concentration in M.
Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg²+ (aq) and a cathode where Cr³+ (aq) is reduced to Cr²+ (aq) at a platinum electrode. Assume all aqueous solutions have a concentration of 1 mol/L. Mg(s)| Mg2+ (aq)|| Cr³+ (aq)| Cr²+ (aq)| Pt(s)
The cell potential of the following cell is determined using an unspecified concentration of acid. What is [H*]given that the measured cell potential is -0.366 V and the anode reduction potential (E') is 0.222 V at 25°C? Agls) | AgCl(s) | CI(1.0 M) || H*(aq, ? M) | H2(g, 1.0 atm) | Pt(s) O 6.1x 102 M O 3.7 x 103M O 4.9x 105 M