For the galvanic (voltaic) cell: Zn(s) + 2TI*(aq)→ 2TI(s) + Zn2* (aq) E cell = 0.42 V If the standard reduction potential for Zn2*(aq) + 2e¬Zn(s) E° red = 1. 0.76 V what is the standard reduction potential for TI*(aq) + e¯-TI(s) E°red = ? V %3D Periodic Table and Datasheet Select one: O a. -0.34 V Ob.-0.17 V O C. +0.17 V O d. +0.34 V

Calculate the [Ni2+] in the following galvanic cell, given that the measured voltage of the cell is 1.120 V at 25oC.   Ni(s) | Ni2+(aq) ( ? M) || Ag+(aq) (0.84 M) | Ag(s)         Ni2+(aq)  +  2 e-  →  Ni(s)    Eo = -0.257 V       Ag+(aq)  +  e-  →  Ag(s)       Eo = 0.800 V   Your answer should have 2 significant figures.

The cell notation for a galvanic cell is shown below. What is the oxidizing agent? Al(s)|A3+(aq)||Au³+(aq)|Au(s) O Al Au3+ O A13+ O Au

Using the provided standard reduction potentials, which of the following cells is an example of a Galvanic cell? A Ag(e)| Ag||Cu*|Cue) Co © Za(e)|Za*|| Cu*|cuke) Au(s)| Au"|| Mn*"|Ma(e) 2+

Calculate E° cell from the tabulated standard reduction potentials for each of the following reactions in aqueous solution. Then calculate AG° and K at 25°C from E° cell' 4 F = 9.65 x 10 J/V•mol e R = 8.314 J/mol•K Acidic solution Standard reduction potential, E (Volts) Cu?" (aq) + e → Cu*(aq) Cu'(ag) + e Cu(s) Mno, (ag) + 8H"(ag) + 5e Mn2"(ag) + 4H,0 0.153 0.521 1.507 Fe"(aq) + e Fe?"(aq) 0.771 Basic solution -1.22 Zn(OH)-(s) + 2e Zn(s) + 4OH(aq) Mno, (aq) + 2H,O + 3e → Mno,(s) + 40H (aq) 0,588 Mn04 + 5FE2+= Mn2+ + 5FE3+ (acidic solution) E°cell = AG° = kJ/mol K =

A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28 Write the balanced overall reaction that powers the cell. Calculate Ecell for the redox reaction. (round to 2 decimal places) What is [Ni²+] when Ecell when reaches 0.03V? (round to 2 sig figs) V What happens at equilibrium? What is Ecell at equilibrium? [Ni²+] at equilibrium: [Co2+] at equilibrium: (round to 2 decimal places) (round to 2 sig figs) (round to 2 sig figs) V M M M

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e - 2 Br (aq) =+1.065 V ʼred MnO,(aq)+2 H,O(1)+3e MnO,(s)+4 ОН (аq) E=+0.59 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Sketch  a galvanic cell  ( immersed in 1M solution)  with the cell notation                     Cr(s)/Cr 3+ (aq) // Cu2+/Cu (s) Please indicate the anode and cathode, the flow of electrons, the reaction in the anode and cathode, overall reaction, and the voltage of the cell- is it spontaneous

Using the following standard reduction potentials, 34 Fe *(aq) + e - Fe2*(aq) Ni2*(ag) + 2 e -Ni(s) E° = +0.77 V E° = -0.26 V calculate the standard cell potential for the cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions 34, Ni 2*( aq) + 2 Fe 2*( aq) → 2 Fe *( aq) + Ni( s) E° = +1.03, nonspontaneous E° = + 1.03, spontaneous E° = -1.03 V, spontaneous E° = -1.03 V, nonspontaneous

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)