General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
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Question
Chapter 17.11, Problem 17.18P
(a)
Interpretation Introduction
Interpretation:
The balanced equation for corrosion that occurs in the presence of Magnesium has to be given.
Concept Introduction:
Corrosion:
Corrosion is natural process that converts a metal into chemically stable form such as Oxide, hydroxide or Sulphide. It is destruction of metal by chemical or
(b)
Interpretation Introduction
Interpretation:
The balanced equation for corrosion that occurs in the absence of Magnesium has to be given.
Concept Introduction:
Corrosion:
Corrosion is natural process that converts a metal into chemically stable form such as Oxide, hydroxide or Sulphide. It is destruction of metal by chemical or electrochemical reaction with their environment.
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Check out a sample textbook solutionChapter 17 Solutions
General Chemistry: Atoms First
Ch. 17.1 - Describe a galvanic cell that uses the reaction...Ch. 17.2 - Write a balanced equation for the overall cell...Ch. 17.2 - Write the shorthand notation for a galvanic cell...Ch. 17.2 - Prob. 17.4CPCh. 17.3 - The standard cell potential at 25 C is 1.21 V for...Ch. 17.4 - The standard potential for the following galvanic...Ch. 17.5 - Which is the stronger oxidizing agent, Cl2(g) or...Ch. 17.5 - Predict from Table 17.1 whether each of the...Ch. 17.5 - Consider the following table of standard reduction...Ch. 17.6 - Consider a galvanic cell that uses the reaction...
Ch. 17.6 - Consider the following galvanic cell: (a) What is...Ch. 17.7 - What is the pH of the solution in the anode...Ch. 17.8 - Use the data in Table 17.1 to calculate the...Ch. 17.8 - Prob. 17.14PCh. 17.9 - Write a balanced equation for the overall cell...Ch. 17.10 - In what ways are fuel cells and batteries similar,...Ch. 17.10 - Prob. 17.17PCh. 17.11 - Prob. 17.18PCh. 17.12 - Metallic potassium was first prepared by Humphrey...Ch. 17.12 - Predict the half-cell reactions that occur when...Ch. 17.13 - Sketch an electrolytic cell suitable for...Ch. 17.14 - How many kilograms of aluminum can be produced in...Ch. 17.14 - A layer of silver is electroplated on a coffee...Ch. 17.14 - What is the overall cell reaction and cell...Ch. 17.14 - Prob. 17.25PCh. 17 - Prob. 17.26CPCh. 17 - Prob. 17.27CPCh. 17 - Prob. 17.28CPCh. 17 - Sketch a cell with inert electrodes suitable for...Ch. 17 - Prob. 17.30CPCh. 17 - It has recently been reported that porous pellets...Ch. 17 - Consider a Daniell cell with 1.0 M ion...Ch. 17 - Consider the following galvanic cell with 0.10 M...Ch. 17 - Prob. 17.34CPCh. 17 - Consider the following table of standard reduction...Ch. 17 - Prob. 17.36SPCh. 17 - What is the function of a salt bridge in a...Ch. 17 - Prob. 17.38SPCh. 17 - Describe galvanic cells that use the following...Ch. 17 - Write the standard shorthand notation for each...Ch. 17 - Write the standard shorthand notation for each...Ch. 17 - Prob. 17.42SPCh. 17 - Write the standard shorthand notation for a...Ch. 17 - An H2/H+ half-cell (anode) and an Ag+/Ag half-cell...Ch. 17 - A galvanic cell is constructed from a Zn/Zn2+...Ch. 17 - Prob. 17.46SPCh. 17 - Prob. 17.47SPCh. 17 - Prob. 17.48SPCh. 17 - Prob. 17.49SPCh. 17 - Prob. 17.50SPCh. 17 - Prob. 17.51SPCh. 17 - Prob. 17.52SPCh. 17 - Prob. 17.53SPCh. 17 - Prob. 17.54SPCh. 17 - Prob. 17.55SPCh. 17 - Prob. 17.56SPCh. 17 - Prob. 17.57SPCh. 17 - Prob. 17.58SPCh. 17 - Prob. 17.59SPCh. 17 - Prob. 17.60SPCh. 17 - Prob. 17.61SPCh. 17 - Prob. 17.62SPCh. 17 - Prob. 17.63SPCh. 17 - Prob. 17.64SPCh. 17 - Calculate E and G (in kilojoules) for the cell...Ch. 17 - Prob. 17.66SPCh. 17 - Prob. 17.67SPCh. 17 - Use the data in Appendix D to predict whether the...Ch. 17 - Use the data in Appendix D to predict whether the...Ch. 17 - Prob. 17.70SPCh. 17 - What reaction can occur, if any, when the...Ch. 17 - Consider a galvanic cell that uses the reaction...Ch. 17 - Prob. 17.73SPCh. 17 - Prob. 17.74SPCh. 17 - Prob. 17.75SPCh. 17 - Prob. 17.76SPCh. 17 - What is the Fe2+: Sn2+ concentration ratio in the...Ch. 17 - The Nernst equation applies to both cell reactions...Ch. 17 - Prob. 17.79SPCh. 17 - Prob. 17.80SPCh. 17 - Prob. 17.81SPCh. 17 - Prob. 17.82SPCh. 17 - Prob. 17.83SPCh. 17 - Prob. 17.84SPCh. 17 - Prob. 17.85SPCh. 17 - Prob. 17.86SPCh. 17 - Prob. 17.87SPCh. 17 - Calculate the equilibrium constant at 25 C for the...Ch. 17 - Prob. 17.89SPCh. 17 - For a lead storage battery: (a) Sketch one cell...Ch. 17 - Prob. 17.91SPCh. 17 - Prob. 17.92SPCh. 17 - Prob. 17.93SPCh. 17 - Prob. 17.94SPCh. 17 - Prob. 17.95SPCh. 17 - Prob. 17.96SPCh. 17 - Prob. 17.97SPCh. 17 - Prob. 17.98SPCh. 17 - (a)Sketch a cell with inert electrodes suitable...Ch. 17 - List the anode and cathode half-reactions that...Ch. 17 - Prob. 17.101SPCh. 17 - Prob. 17.102SPCh. 17 - Predict the anode, cathode, and overall cell...Ch. 17 - Prob. 17.104SPCh. 17 - Prob. 17.105SPCh. 17 - How many hours are required to produce 1.00 103...Ch. 17 - Prob. 17.107SPCh. 17 - Prob. 17.108SPCh. 17 - Prob. 17.109SPCh. 17 - Prob. 17.110CHPCh. 17 - Prob. 17.111CHPCh. 17 - Prob. 17.112CHPCh. 17 - Prob. 17.113CHPCh. 17 - Prob. 17.114CHPCh. 17 - Prob. 17.115CHPCh. 17 - Prob. 17.116CHPCh. 17 - Prob. 17.117CHPCh. 17 - Prob. 17.118CHPCh. 17 - The sodium-sulfur battery has molybdenum...Ch. 17 - When suspected drunk drivers are tested with a...Ch. 17 - Consider the addition of the following...Ch. 17 - The following galvanic cell has a potential of...Ch. 17 - A galvanic cell has a silver electrode in contact...Ch. 17 - Prob. 17.124CHPCh. 17 - Prob. 17.125CHPCh. 17 - Prob. 17.126CHPCh. 17 - For the following half-reaction, E = 1.103 V:...Ch. 17 - Prob. 17.128CHPCh. 17 - Prob. 17.129CHPCh. 17 - Prob. 17.130MPCh. 17 - Prob. 17.131MPCh. 17 - Prob. 17.134MPCh. 17 - Prob. 17.135MPCh. 17 - Prob. 17.136MPCh. 17 - Prob. 17.137MPCh. 17 - Experimental solid-oxide fuel cells that use...Ch. 17 - The half-reactions that occur in ordinary alkaline...Ch. 17 - Gold metal is extracted from its ore by treating...Ch. 17 - Consider the redox titration of 100.0 mL of a...
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- 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)?arrow_forwardIn some old European churches, the stained-glass windowshave so darkened from corrosion and age that hardly anylight comes through. Microprobe analysis showed that tinycracks anddefects on the glass surface were enriched ininsoluble Mn(III) and Mn(IV) compounds. From AppendixE, suggest a reducing agent and conditions that might successfullyconvert thesecompounds to soluble Mn(II) withoutsimultaneously reducing Fe(III) (which gives the glassits colors) to Fe(II). Take MnO2 as representative of theinsoluble Mn(III) and Mn(IV) compounds.arrow_forwardCalculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)arrow_forward
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