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(a)
Interpretation:
The overall balanced
Concept introduction:
Standard Gibbs free energy of a reaction is used check whether the reaction is spontaneous or not. If the value of
![Check Mark](/static/check-mark.png)
Answer to Problem 8.11E
The overall balanced electrochemical reaction is as follows,
The value of
Explanation of Solution
The given reaction is represented as,
From Table
The number of moles of electrons transferred in the above reaction is
From Table
The above equation is reversed and the value of
The number of moles of electrons transferred in the above reaction is
The relation between standard Gibbs free energy and standard electrical potential is represented as,
Where,
•
•
•
•
Substitute the values of the standard reduction potential of the reaction (1),
The value
Substitute the values of the standard oxidation potential of the reaction (2),
The value
The balanced overall electrochemical reaction is obtained by multiplying chemical equation (1) by
Therefore, the value
The number of electrons transferred in the overall reaction is
Rearrange the equation (3) for the value of
Substitute the values of
The value of
The overall balanced electrochemical reaction is as follows,
The value of
(b)
Interpretation:
The overall balanced electrochemical reaction and the values of
Concept introduction:
Standard Gibbs free energy of a reaction is used check whether the reaction is spontaneous or not. If the value of
![Check Mark](/static/check-mark.png)
Answer to Problem 8.11E
The overall balanced electrochemical reaction is as follows,
The value of
Explanation of Solution
The given reaction is represented as,
From Table
The above equation is reversed and the value of
The number of moles of electrons transferred in the above reaction is
From Table
The number of moles of electrons transferred in the above reaction is
The relation between standard Gibbs free energy and standard electrical potential is represented as,
Where,
•
•
•
•
Substitute the values of the standard oxidation potential of the reaction (4),
The value
Substitute the values of the standard reduction potential of the reaction (5),
The value
The balanced overall electrochemical reaction is obtained by multiplying chemical equation (5) by
Therefore, the value
The number of electrons transferred in the overall reaction is
Rearrange the equation (3) for the value of
Substitute the values of
The value of
The overall balanced electrochemical reaction is as follows,
The value of
(c)
Interpretation:
The overall balanced electrochemical reaction and the values of
Concept introduction:
Standard Gibbs free energy of a reaction is used check whether the reaction is spontaneous or not. If the value of
![Check Mark](/static/check-mark.png)
Answer to Problem 8.11E
The overall balanced electrochemical reaction is as follows,
The value of
Explanation of Solution
The given reaction is represented as,
From Table
The above equation is reversed and the value of
The number of moles of electrons transferred in the above reaction is
From Table
The number of moles of electrons transferred in the above reaction is
The relation between standard Gibbs free energy and standard electrical potential is represented as,
Where,
•
•
•
•
Substitute the values of the standard reduction potential of reaction (6),
The value
Substitute the values of the standard reduction potential of reaction (7),
The value
Add chemical equation (6) and chemical equation (7) to obtain the balanced overall electrochemical reaction. The formation of overall balanced chemical equation is represented as,
Therefore, the value
The number of electrons transferred in the overall reaction is
Rearrange the equation (3) for the value of
Substitute the values of
The value of
The overall balanced electrochemical reaction is as follows,
The value of
(d)
Interpretation:
The overall balanced electrochemical reaction and the values of
Concept introduction:
Standard Gibbs free energy of a reaction is used check whether the reaction is spontaneous or not. If the value of
![Check Mark](/static/check-mark.png)
Answer to Problem 8.11E
The overall balanced electrochemical reaction is as follows,
The value of
Explanation of Solution
The given reaction is represented as,
From Table
The number of moles of electrons transferred in the above reaction is
From Table
The above equation is reversed and the value of
The number of moles of electrons transferred in the above reaction is
The relation between standard Gibbs free energy and standard electrical potential is represented as,
Where,
•
•
•
•
Substitute the values of the standard reduction potential of the reaction (8),
The value
Substitute the values of the standard oxidation potential of the reaction (9),
The value
Add chemical equation (8) and chemical equation (9) to obtain the balanced overall electrochemical reaction. The formation of overall balanced chemical equation is represented as,
The value
The number of electrons transferred in the overall reaction is
Rearrange the equation (3) for the value of
Substitute the values of
The value of
The overall balanced electrochemical reaction is as follows,
The value of
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Chapter 8 Solutions
Physical Chemistry
- An 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_forward1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how long must you electrolyze a solution if the current passing through the circuit is 2.00 amps? 483 seconds 4.83 104 seconds 965 seconds 1450 secondsarrow_forwardOrder the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq).arrow_forward
- Consider the following cell running under standard conditions: Fe(s)Fe2+(aq)Al3+(aq)Al(s) a Is this a voltaic cell? b Which species is being reduced during the chemical reaction? c Which species is the oxidizing agent? d What happens to the concentration of Fe3+(aq) as the reaction proceeds? e How does the mass of Al(s) change as the reaction proceeds?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_forwardAt 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.arrow_forward
- Consider 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_forwardAt 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.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_forward
- 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_forwardFor 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_forwardThe 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_forward
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