
General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
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Chapter 17, Problem 17.83SP
Interpretation Introduction
Interpretation:
The value of
Concept Introduction:
Standard cell potential and equilibrium constant:
The standard cell potential related to the free-energy is given by the equation,
The free-energy change is also related to equilibrium constant by the equation,
Combine both the equations,
Where,
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Predict the major products of this reaction:
་ ་
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H
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Δ
excess
Note that the second reactant is used in excess, that is, there is much more of the second reactant than the first.
If there won't be any products, just check the box under the drawing area instead.
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A student claims the right-hand side of the reaction in the drawing area below shows the product of a Claisen condensation.
• If the student is correct, complete the reaction by adding the necessary organic reactants to the left-hand side, and by adding any necessary reagents and
reaction conditions above and below the arrow.
• If the student is incorrect, because it's not possible to obtain this product from a Claisen condensation, check the box under the drawing area instead.
those that will minimize any byproducts or competing
• Note for advanced students: If you have a choice, use the most efficient reactants and reagents
reactions.
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☐
: ☐
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Click and drag to start
drawing a structure.
identify the relationship between the
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H
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Chapter 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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