Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Cl, (g) + 2 e- 2 Cr (aq) 1.360 02(g) + 4 H30*(aq) + 4 e" - 6 H2O(1) 1.229 →H2(g) + 2 OH (aq) |-0.828 |-0.763 2 H20(1) + 2 e Zn* (aq) + 2 e – Zn (s) A 0.143 M neutral aqueous ZnCl, solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: Half-reaction at cathode: (b) What is the expected decomposition potential? +

Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Cl, (g) + 2 e- 2 Cr (aq) 1.360 02(g) + 4 H30(aq) + 4 e" - 6 H2O(1) 1.229 →H2(g) + 2 OH (aq) |-0.828 |-0.763 2 H20(1) + 2 e Zn (aq) + 2 e – Zn (s) A 0.143 M neutral aqueous ZnCl, solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: Half-reaction at cathode: (b) What is the expected decomposition potential? +

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 150CP: Given the following two standard reduction potentials, solve for the standard reduction potential of...

See similar textbooks

Similar questions

Given the following two standard reduction potentials, solve for the standard reduction potential of the half-reaction M3++eM2+ (Hint: You must use the extensive property G to determine the standard reduction potential.)
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
Consider only the species (at standard conditions) Na+, Cl, Ag+, Ag, Zn2+, Zn, Pb in answering the following questions. Give reasons for your answers. (Use data from Table 17-1.) a. Which is the strongest oxidizing agent? b. Which is the strongest reducing agent? c. Which species can be oxidized by SO42 (aq) in acid? d. Which species can be reduced by Al(s)?
The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)
The standard potential for the reduction of AgSCN is 0.0895 V. AgSCN(s)+eAg(s)+SCN(aq) Find another electrode potential to use together with the above value and calculate Kspfor AgSCN.
At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)