MISSED THIS? Read Section 20.4 (Pages 903-913); Watch KCY 20.4 Decide whether or not each of the following metals dissolves in 1 M HNO₂. For those metals that do dissolve, enter a balanced net lonic redox reaction showing what happens when the metal dissolves Consider the table of standard electrode potentials at 25 C Reduction hat-reaction B (V) 1.50 NO(g) + 2H₂O(1) 096 0.34 0 -0.76 -1.06 Au (aq) + 3e NOS (aq) + 4H(aq) + 3e Cu (aq) +201 21' (aq) + Za (aq) + 2e → Zn(s) AP (aq) + 3+ Al(a) →Au(n) → Cu(s) H₂(g) Y Part A Cu Express your answer as a balanced net ionic equation including phase NOREACTION if there is no reaction. | ΑΣΦ X Submit A chemical reaction does not occur for this question . Previous Answers Request Answer 4

MISSED THIS? Read Section 20.4 (Pages 903-913); Watch KCY 20.4 Decide whether or not each of the following metals dissolves in 1 M HNO₂. For those metals that do dissolve, enter a balanced net lonic redox reaction showing what happens when the metal dissolves Consider the table of standard electrode potentials at 25 C Reduction hat-reaction B (V) 1.50 NO(g) + 2H₂O(1) 096 0.34 0 -0.76 -1.06 Au (aq) + 3e NOS (aq) + 4H(aq) + 3e Cu (aq) +201 21' (aq) + Za (aq) + 2e → Zn(s) AP (aq) + 3+ Al(a) →Au(n) → Cu(s) H₂(g) Y Part A Cu Express your answer as a balanced net ionic equation including phase NOREACTION if there is no reaction. | ΑΣΦ X Submit A chemical reaction does not occur for this question . Previous Answers Request Answer 4

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 160MP

See similar textbooks

Similar questions

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 metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
Consider a battery made from one half-cell that consists of a capper electrode in 1 M CuSO4 solution and another half—cell that consists of a lead electrode in 1 M Pb(NO3)2 solution. (a) What are the reactions at the anode, cathode, and the overall reaction? (b) What is the standard cell potential for the battery? (c) Most devices designed to use dry-cell batteries can operate between 1.0 and 1.5 V. Could this tell he used to make a battery that could replace a dry-cell battery? Why or why not. (d) Suppose sulfuric acid is added to the half—cell with the lead electrode and some PbSO4(s) forms. Would the cell potential increase, decrease, or remain the same?
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.
Identify the reaction at the anode, reaction at the cathode, the overall reaction, and the approximate potential required for the electrolysis of the following molten salts. Assume standard states and that the standard reduction potentials in Appendix L are the same as those at each of the melting points. Assume the efficiency is 100%. (a) CaCl2. (b) LiH. (c) AlCl3. (d) CrBr3
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.)
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)?
An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.00 M separated by a porous disk from a compartment with a copper metal electrode immersed in a solution of 10.00 M NH3 that also contains 2.4 103 M Cu(NH3)42+. The equilibrium between Cu2+ and NH3 is: Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013 and the two cell half-reactions are: Assuming Ag+ is reduced, what is the cell potential at 25C?