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A galvanic cell is constructed using a zinc electrode immersed in a 1.0 M Zn2+ solution...
Q. Consider a galvanic cell with a zinc electrode immersed in 1.0M Zn2+ and a silver electrode immersed in 1.0M Ag+. Which of the electrodes is the anode? Zn2 + 2e- --> Zn E° = -0.76 V Ag+ + e- --> Ag E° = 0.80 V
3. Consider a galvanic cell with a copper electrode immersed in 1.0 M Cu and a silver electrode immersed in 1.0 M Ag Cu +2e-Cu E 0.34 V Ag +e-Ag (1pt) Calculate E° for this cell. a. b. (1pt) Identify the anode and cathode. (1pt) Identify the oxidizing and reducing agent. c.
Consider an electrochemical cell with a zinc electrode immersed in a solution of ZnT and in electrical contact with a silver electrode immersed in a solution of Ag. If the initial concentrations of Zinc and Silver ions are 0.0050 M and 16.00 M respectively, calculate +2 cell
Consider an electrochemical cell with a zinc electrode immersed in a solution of ZnT and in electrical contact with a silver electrode immersed in a solution of Ag. If the initial concentrations of...
For a voltaic (or galvanic) cell using Ag, Ag+ (1.0M) and Zn Zn2+ (1.0 M) half-cells, which of the following statements is incorrect? (a) The zinc electrode is the anode. (b) Electrons will flow through the external circuit from the zinc electrode to the silver electrode. (c) The mass of the zinc electrode will decrease as the cell operates. (d) The concentration of Ag will decrease as the cell operates. (e) Reduction occurs at the zinc electrode as the cell operates.
Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2and a silver electrode immersed in 1.0 M Agt. Zn2+ + 2e- → Zn E° = -0.76 V Agt + e- Ag E = 0.80 V Calculate Eº and AGº for this cell Calculate AGº for the reaction: 2 Zn (g) + O2 (g) + 2 H20 (1) ► 2 Zn2+ (aq) + 4 OH (aq) Reduction Half-Reaction E° (V) O2(g) + 2 H20 (1)+4 e-®4 OH(aq) +0.403...
A galvanic (voltaic) cell consists of an electrode composed of zinc in a 1.0 M zinc ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found here.
Given which of the following sets of thermodynamic parameters is a reaction spontaneous only at higher temperatures? A) ΔH < 0 and ΔS < 0 B) ΔH < 0 and ΔS > 0 C) ΔH > 0 and ΔS > 0 D) ΔH > 0 and ΔS < 0 ---------------------------------------------------------------------------------------------------------------------------- A galvanic cell is constructed using a zinc electrode immersed in a 1.0 M Zn2+ solution and a silver electrode immersed in a 1.0 M Ag+ solution. What is the...
A galvanic cell Crs)Cr2(aq) || Pb2*(a)|Pb( is constructed using a completely immersed Cr electrode that weighs 25.0 g and a Pb electrode immersed in 632 mL of 1.00 M Pb*(aq) solution. A steady current of 0.0719 A is drawn from the cell as the electrons move from the Cr 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)...
A voltaic cell contains two half-cells. One half-cell contains a zinc electrode immersed in a 1.00 M Zn(NO3)2 solution. The second half-cell contains a titanium electrode immersed in a 1.00 M Ti(NO3)3 solution. Zn2+(aq) + 2 e− → Zn(s) E⁰red = −0.762 V Ti3+(aq) + 3 e− → Ti(s) E⁰red = −1.370 V (a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. _____ V (b) Write the overall balanced equation for the...
A galvanic cell Cr(s)|Cr2+(aq) || Cu2+(aq)|Cu(s) is constructed using a completely immersed Cr electrode that weighs 35.4 g and a Cu electrode immersed in 462 mL of 1.00 M Cu2+(aq) solution. A steady current of 0.0795 A is drawn from the cell as the electrons move from the Cr electrode to the Cu 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? s...