a.
Interpretation: Whether the cell potential of given galvanic cell increase, decrease, or remain the same when
Concept Introduction: The measure of energy per unit charge which is available from the
Nernst equation gives the relationship between standard reduction potential,
Where
This equation is specified at room temperature,
a.
Answer to Problem 111AE
The value of
Explanation of Solution
Given:
The half reactions of standard galvanic cell as:
The reduction potential values for the half reactions of standard galvanic cell is:
Since, the reduction potential value of silver is greater than copper so, the silver will undergo reduction and copper will undergo oxidation so, the half-reactions are written as:
To balance the charge on both sides, the reduction reaction,
Adding both the reactions to get the overall reactions as:
So, the overall balanced reaction for the galvanic cell is:
Now, according to Nernst equation at room temperature,
Now, on adding
b.
Interpretation: Whether the cell potential of given galvanic cell increase, decrease, or remain the same when
Concept Introduction: The measure of energy per unit charge which is available from the redox reactions to carry out the reaction is said to be cell potential.
Nernst equation gives the relationship between standard reduction potential,
Where
This equation is specified at room temperature,
b.
Answer to Problem 111AE
The value of
Explanation of Solution
According to Nernst equation at room temperature,
Now, on adding
c.
Interpretation: Whether the cell potential of given galvanic cell increase, decrease, or remain the same when
Concept Introduction: The measure of energy per unit charge which is available from the redox reactions to carry out the reaction is said to be cell potential.
Nernst equation gives the relationship between standard reduction potential,
Where
This equation is specified at room temperature,
c.
Answer to Problem 111AE
The value of
Explanation of Solution
According to Nernst equation at room temperature,
Now, on adding
d.
Interpretation: Whether the cell potential of given galvanic cell increase, decrease, or remain the same when water is added to both half-cell compartment until the volume of solution is doubled.
Concept Introduction: The measure of energy per unit charge which is available from the redox reactions to carry out the reaction is said to be cell potential.
Nernst equation gives the relationship between standard reduction potential,
Where
This equation is specified at room temperature,
d.
Answer to Problem 111AE
The value of
Explanation of Solution
According to Nernst equation at room temperature,
Now, on adding water to both half-cell compartment until the volume of solution gets doubled it will result in decreasing the concentration of both the ions, silver ion,
e.
Interpretation: Whether the cell potential of given galvanic cell increase, decrease, or remain the same when silver electrode is replaced with platinum electrode:
Concept Introduction: The measure of energy per unit charge which is available from the redox reactions to carry out the reaction is said to be cell potential.
Nernst equation gives the relationship between standard reduction potential,
Where
This equation is specified at room temperature,
e.
Answer to Problem 111AE
The value of
Explanation of Solution
Given:
The half reactions of standard galvanic cell as:
The reduction potential values for the half reactions of standard galvanic cell is:
Since, the reduction potential value of platinum is greater than copper so, the platinum will undergo reduction and copper will undergo oxidation so, the half-reactions are written as:
Adding both the reactions to get the overall reactions as:
So, the overall balanced reaction for the galvanic cell is:
Now, according to Nernst equation at room temperature,
So, on replacing the silver electrode by platinum electrode, the
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Chapter 11 Solutions
Chemical Principles
- You want to set up a series of voltaic cells with specific cell potentials. A Zn2+(aq, 1.0 M)| Zn(s) half-cell is in one compartment. Identify several half-cells that you could use so that the cell potential will be close to (a) 1.1 V and (b) 0.50 V. Consider cells in which the zinc cell can be either the cathode or the anode.arrow_forwardFour voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode. The second half-cell is one of the following: (i) Cr3+(aq, 1.0 M)|Cr(s) (ii) Fea+(aq, 1.0M)|Fe(s) (iii) Cu2+(aq, 1.0M)|Cu(s) (iv) Mg2+(aq, 1.0M)|Mg(s) (a) In which of the voltaic cells does the hydrogen electrode serve as the cathode? (b) Which voltaic cell produces the highest potential? Which produces the lowest potential?arrow_forwardYou have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.arrow_forward
- The half cells Sn2+(aq) |Sn(s) and Cl2(g) |Cl(aq) are linked to create a voltaic cell. (a) Write equations for the oxidation and reduction half-reactions and for the overall (cell) reaction. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the ______ electrode to the ____ electrode. Negative ions move in the salt bridge from the _____ half-cell to the _____ half-cell.arrow_forwardA voltaic cell is constructed using the reaction of chromium metal and iron(II) ions. 2 Cr(s) + 3 Fe2+(aq) 2 Cr3+(aq) + 3 Fe(s) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ________ half-cell to the ______ half-cell. The half-reaction at the anode is _______ and that at the cathode is ________.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
- From the information provided, use cell notation to describe the following systems: (a) In one half-cell, a solution of Pt(NO3)2 forms Pt metal, while in the other half-Cell, Cu metal goes into a.Cu(NO3)2 solution with all solute concentrations 1 M. (b) The cathode consists of a gold electrode in a 0.55 M Au(NO3)3 solution and the anode is a magnesium electrode in 0.75 M Mg(NO3)2 solution. (c) One half-cell consists of a silver electrode in a 1 M AgNO3 solution, and in the other half-cell, a copper Electrode in 1 M Cu(NO3)2 is oxidized.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_forwardA voltaic cell is constructed using the reaction Mg(s) + 2H+(aq) Mg2+(aq) + H2(g) (a) Write equations for the oxidation and reduction half-reactions. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ______ half-cell to the ______ half-cell. The half-reaction at the anode is ____, and that at the cathode is _____.arrow_forward
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