Concept explainers
(a)
Interpretation:
The ratio of molarity of the ions in the given concentration cells required to have
Concept introduction:
The type of
Answer to Problem 8.35E
The ratio of
Explanation of Solution
The given concentration cell is,
For a concentration cell, standard electrode potential
The electrode potential at the given concentration can be calculated by using the Nernst equation as shown below.
Where,
•
•
•
•
•
•
Substitute the values of given potential, standard electrode potential and concentration of the species in the formula.
Solve for the value of ratio of
Thus, the ratio of
The ratio of
(b)
Interpretation:
The ratio of molarity of the ions in the given concentration cells required to have
Concept introduction:
The type of electrochemical cells which is comprised of two same electrodes but different concentrations or pressures is known as concentration cell.
Answer to Problem 8.35E
The ratio of
Explanation of Solution
The given concentration cell is,
For a concentration cell standard electrode potential
The electrode potential at the given concentration can be calculated by using the Nernst equation as shown below.
Where,
•
•
•
•
•
•
Substitute the values of given potential, standard electrode potential and concentration of the species in the formula.
Solve for the value of ratio of
Thus, the ratio of
The ratio of
(c)
Interpretation:
The ratio of molarity of the ions in the given concentration cells required to have
Concept introduction:
The type of electrochemical cells which is comprised of two same electrodes but different concentrations or pressures is known as concentration cell.
Answer to Problem 8.35E
The ratio of
Explanation of Solution
The given concentration cell is,
For a concentration cell standard electrode potential
The electrode potential at the given concentration can be calculated by using the Nernst equation as shown below.
Where,
•
•
•
•
•
•
Substitute the values of given potential, standard electrode potential and concentration of the species in the formula.
Solve for the value of ratio of
Thus, the ratio of
The ratio of
(d)
Interpretation:
The answers are to be compared and similarities or differences are to be stated.
Concept introduction:
The type of electrochemical cells which is comprised of two same electrodes but different concentrations or pressures is known as concentrations cells.
Answer to Problem 8.35E
The ratio of molarities is equal in case of
Explanation of Solution
The ratio of molarities is equal in case of
The ratio of molarities is equal in case of
Want to see more full solutions like this?
Chapter 8 Solutions
Physical Chemistry
- For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)arrow_forwardCalculate the standard cell potential of the cell corresponding to the oxidation of oxalic acid, H2C2O4, by permanganate ion. MnO4. 5H2C2O4(aq)+2MnO4(aq)+6H+(aq)10CO2(g)+2Mn2+(aq)+8H2O(l) See Appendix C for free energies of formation: Gf for H2C2O4(aq) is 698 kJ.arrow_forwardFor each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)arrow_forward
- a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).arrow_forwardConsider 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.arrow_forwardAn 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)?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning