In a voltaic cell the cathode is an Ag+ [1.00 M/Ag(s)] half-cell. The anode is a standard hydrogen electrode immersed in a buffer solution containing 0.10 M benzoic acid (C6H5COOH) and 0.050 M sodium benzoate (C6H5COONa). The measured cell voltage is 1.030 V. Calculate pKa for benzoic acid.

Consider an electrochemical cell made up of Au Au* and Co²+ | Co³+ half-cells. Part 1 of 2 Write the equation for the cell reaction that occurs under standard-state conditions. Be sure to include the physical state of each species in the reaction. Part 2 of 2 E = ローロ V 00 Calculate the standard emf of a cell that uses the Au Au and Co²+ | Co³+ half-cell reaction at 25 °C. Round your answer to 2 significant digits. Note: Reference the Standard reduction potentials at 25 °C table for additional information. 09 S

Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmium.   In(s)||In3+(aq)‖‖Cd2+(aq)||Cd(s)In(s)⁢|In3+⁢(aq)‖Cd2+⁢(aq)|Cd(s)   anode:   cathode:   net cell reaction:

Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these

Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K.   Cd2+(aq) + 2e–   →  Cd(s)                     E° = –0.403 V                         Pb2+(aq) + 2e–   →   Pb(s)                     E° = –0.126 V     E°cell = ______________     Ecell = ______________

Calculate Eu for the following cell: Pt(s) | H₂(g) | H *(aq) || Pb2+ (aq) | PbSO4(s) | Pb(s) given the following standard reduction potentials. 2 H(aq) + 2e →→ H₂(g) PbSO4(s) + 2e →→ Pb(s) + SO42 (aq) O a. -0.712 V O b. +0.356 V O c. -0.356 V O d. +0.712 V O e. -0.178 V E° = 0.000 V E = -0.356 V

What is the cell potential for a voltaic cell having one electrode composed of a Zn strip dipped in a 0.034 M Zn(NO)(aq) solution and the other electrode composed of a Zn strip dipped into a 0.414 M Zn(NO)(aq) solution? Assume all other cell components are in place and the temperature is 25.0°C.   To produce 1.21 kg of solid potassium from molten KCl, how many hours must 0.721 amps be passed through the KCl?   How many hours will you have to electrolyze the forks to apply 0.500 g of Ag to each one? Your electrolysis device operates at a current of 3.75 amps.

A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3 Cu2+(aq)+2A1 (s) → 3 Cu (s) + 2A13+ (aq) Suppose the cell is prepared with 5.34 M Cu 2+ in one half-cell and 2.28 M A13+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ☐ x10 μ ロ・ロ

What is the overall cell reaction and the standard cell potential of a galvanic cell employing the following half-reactions ? NiO 2(s) +2H 2 O+2e^ -. ---> Ni(OH) 2(s) +2OH^- (aq) E ^ 0 = 0.49V   Fe(OH) 2(s) +2e^ - ----> Fe (s) +2OH^- (aq) E ^ 0 = - 0.88 V

Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. Identify the reactions with K > 1 among the following redox reactions. Write the line representations for the Galvanic cells, indicating the anode and 1. cathode. a. Cl2 + Br → Ct + Br2 b. Mnoa + H* + Ce → Cet + Mn2 + H20