2. Why would a sacrificial anode made of lithium metal be a bad choice despite ts E•Li+/Li=-3.04 V, which appears to be able to protect all the other metals listed in che standard reduction potential table?

2. Why would a sacrificial anode made of lithium metal be a bad choice despite ts E•Li+/Li=-3.04 V, which appears to be able to protect all the other metals listed in che standard reduction potential table?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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indTap - Cengage Learni.. Courses Transfer Course Equivalen. OWLV2 | Online teaching Homepage [Review Topics] [References] Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg*(aq) + 2I°(aq)→ Hg(1) + I½(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG° for this reaction would be O than zero. Submit Answer Retry Entire Group 9 more group attempts remaining Previou Email Instruc Cengage Learning | Cengage Technical Support DII DD F9 F10 F11 F4 ES F6 F7 F8 F3 $ % & 4 5 6 7 8 9
please explain and answer all parts or better to leave it
Using data from the Standard Reduction Potentials table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). (Use the appropriate symbol to separate substances in the list.) chemPad 2+ Cd²+, K+, Cr³+, Au³+, 103¯¯, and Ba 2+ XX→→ Need Help? Read It Supporting Materials Periodic Table Help Greek Constants & Factors Supplemental Data
7. What current density is necessary to get a Cu plating rate of 0.005 mm per minute? 8. What is the material removal rate for Fe if the corrosion current density is 15 HA/cm2? 9. Assuming the anodic Tafel constant is 0.1 V, how much will the corrosion rate increase if the electrode is polarized 0.2 V in the positive direction? 10. Assuming the Tafel constant is 0.1 V, how much must we cathodically polarize a corroding sample to reduce the corrosion rate by a factor of 50?
Refer to the following table: O Hint: Recall E cell A (A) -0.34 V B (B) -0.52 V Half-reaction = Ered + Ni2+ + 2e → Ni Cd2+ + 2e → Cd Cute Cu La³+ + 3e → La Fe³+ + e Fe²+ The standard cell potential for the galvanic cell denoted by the line notation below is 0.86 V. What is the standard reduction potential for the oxidation half-reaction? Tl(s) | Tl* (aq) || Cu* (aq) | Cu(s) (C) +0.34 V Ered° (V) E ox -0.23 -0.40 0.52 -2.37 0.77 (D) +1.38 V
How much solid gallium can you plate if you pass a current of 0.570 amps through a solution of gallium (III) oxide in concentrated sodium hydroxide for 50 minutes? HINT: Molar mass of gallium = 69.723 g/mol Amount of Ga = g
Do not have to answer any questions. JUST WRITE THE OBJECTIVES IN YOUR OWN RODS: Objective: To measure Ecel for several voltaic cells and determine the standard potential for each half cell. To determine Ksp of AgCl and the K of [Cu(NH3)4]*.
If 12.0 g of Cr are plated from an aqueous solution containing Cr* ions using a current of 3.50 amps, how many minutes did the current flow? Recall the faraday is 96,500 coulombs/mole and the atomic mass of Cr= 52.00
#73
A concentration cell similar to the one shown is composed of two Sn electrodes and solutions of different Sn2+ concentrations. The left compartment contains 0.974 M Sn2+ , and the right compartment contains 0.677 M Sn2+ .Calculate the cell potential for this reaction at 298 K. volts In this tin concentration cell, the compartment on the left is the , and the compartment on the right is the .
A chromium metal was deposited coming from a solution of Cr+3. The amount of the saidmetal deposited weighs 2.19 g. The process is made possible through a current of 35.2Amperes in electrolyte cell. Determine the following:a. How much charge (in C) is required?b. How long (in min) would it take for the reaction to occur?