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Concept explainers
(a)
Interpretation:
The ratio of molarity of the ions in the given concentration cells required to have
Concept introduction:
The type of
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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.
![Check Mark](/static/check-mark.png)
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.
![Check Mark](/static/check-mark.png)
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.
![Check Mark](/static/check-mark.png)
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
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Chapter 8 Solutions
Physical Chemistry
- 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)?arrow_forwardAn electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?arrow_forwardWhat is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?arrow_forward
- The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).arrow_forwardCalcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a) How many joules of electrical energy are required to obtain 12.0 1b of calcium? (b) What is the cost of the electrical energy obtained in (a) if electrical energy is sold at the rate of nine cents per kilowatt hour?arrow_forwardAn electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?arrow_forward
- 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_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) Cu2+(aq)+Ni(s)Cu(s)+Ni2+(aq) (b) 2Ag(s)+Cl2(g)2AgCl(s) (c) Cl2(g)+2I(aq)2Cl(aq)+I2(s)arrow_forwarda 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_forward
- Consider the electrolysis of water in the presence of very dilute H2SO4. What species is produced at the anode? Atthe cathode? What are the relative amounts of the speciesproduced at the two electrodes?arrow_forwardConsider the following cell reaction at 25C. 2Cr(s)+3Fe2+(aq)2Cr3+(aq)+3Fe(s) Calculate the standard cell potential of this cell from the standard electrode potentials, and from this obtain G for the cell reaction. Use data in Appendix C to calculate H; note that Cr(H2O)63+(aq) equals Cr3+(aq). Use these values of H and G to obtain S for the cell reaction.arrow_forwardA voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3.The other half cell consists of an inert platinum wire in an aqueous solution containing Fe2+(aq) and Fe3+(aq). (a) Calculate the cell potential, assuming standard conditions. (b) Write the net ionic equation for the reaction occurring in the cell. (c) Which electrode is the anode and which is the cathode? (d) If [Ag+] is 0.10 M, and [Fe2+] and [Fe3+] are both 1.0 M, what is the cell potential? Is the net cell reaction still that used in part (a)? If not, what is the net reaction under the new conditions?arrow_forward
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