ISSED THIS? Read Section 20.5 (Pages 913-917); Watch KCV 0.5, IWE 20.6. se tabulated half-cell potentials to calculate AG for each of the allowing reactions at 25 °C. ▼ Part B O₂(g) + 2H₂O(1) +2Cu(s) →40H (aq) + 2Cu²+ (aq) Express the energy change in kilojoules to one significant figure. ▸ View Available Hint(s) AGE= -20 kJ Submit Previous Answers ✓ Correct There are fewer electrons transferred and the standard cell potential is smaller in magnitude when comparing this reaction to the one in Part A, so this redox reaction is less spontaneous than that of Part A. Part C Br2 (1)+21 (aq) → 2Br (aq) + I₂(s) Express the energy change in kilojoules to two significant figures. ▸ View Available Hint(s) [5] ΑΣΦ AG-11 Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining ? kJ

ISSED THIS? Read Section 20.5 (Pages 913-917); Watch KCV 0.5, IWE 20.6. se tabulated half-cell potentials to calculate AG for each of the allowing reactions at 25 °C. ▼ Part B O₂(g) + 2H₂O(1) +2Cu(s) →40H (aq) + 2Cu²+ (aq) Express the energy change in kilojoules to one significant figure. ▸ View Available Hint(s) AGE= -20 kJ Submit Previous Answers ✓ Correct There are fewer electrons transferred and the standard cell potential is smaller in magnitude when comparing this reaction to the one in Part A, so this redox reaction is less spontaneous than that of Part A. Part C Br2 (1)+21 (aq) → 2Br (aq) + I₂(s) Express the energy change in kilojoules to two significant figures. ▸ View Available Hint(s) [5] ΑΣΦ AG-11 Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining ? kJ

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 76AP

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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)?
Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 C. Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s) a. Write a balanced equation for the reaction that occurs at the cathode. b. Write a balanced equation for the reaction that occurs at the anode. c. Write a balanced chemical equation for the overall reaction. d. Determine the potential (in volts) of the cell.
Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.
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.
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?