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(a)
Interpretation:
The oxidation half-cell reaction for the
Concept introduction:
In an
The reduction is defined as a process in which the gain of electrons occurs, whereas oxidation is defined as the process of loss of electrons. The substance that is oxidized is a reducing agent and the substance that is reduced is an oxidizing agent.
(b)
Interpretation:
The reduction half-cell reaction for the redox reaction of tin and cobalt sulfate is to be stated.
Concept introduction:
In an electrochemical cell, two electrodes are connected by a wire and electrons are free to move between two compartments. Each compartment is known as a half-cell.
The reduction is defined as a process in which the gain of electrons occurs, whereas oxidation is defined as the process of loss of electrons. The substance that is oxidized is a reducing agent and the substance that is reduced is an oxidizing agent.
(c)
Interpretation:
The anode and cathode for the redox reaction of tin and cobalt sulfate is to be stated.
Concept introduction:
In an electrochemical cell, two electrodes are connected by a wire and electrons are free to move between two compartments. Each compartment is known as a half-cell.
The reduction is defined as a process in which the gain of electrons occurs, whereas oxidation is defined as the process of loss of electrons. The substance that is oxidized is a reducing agent and the substance that is reduced is an oxidizing agent.
(d)
Interpretation:
The direction of electron flow for the redox reaction of tin and cobalt sulfate is to be stated.
Concept introduction:
In an electrochemical cell, two electrodes are connected by a wire and electrons are free to move between two compartments. Each compartment is known as a half-cell.
The reduction is defined as a process in which the gain of electrons occurs, whereas oxidation is defined as the process of loss of electrons. The substance that is oxidized is a reducing agent and the substance that is reduced is an oxidizing agent.
(e)
Interpretation:
The direction of
Concept introduction:
In an electrochemical cell, two electrodes are connected by a wire and electrons are free to move between two compartments. Each compartment is known as a half-cell.
The reduction is defined as a process in which the gain of electrons occurs, whereas oxidation is defined as the process of loss of electrons. The substance that is oxidized is a reducing agent and the substance that is reduced is an oxidizing agent.
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Chapter 17 Solutions
EBK INTRODUCTORY CHEMISTRY
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- At 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_forwardFor the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+ (aq), why can’t you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing CuCl2(aq) and ZnCl2(aq)?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
- A 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_forwardThe 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_forwardConsider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?arrow_forward
- At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)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_forwardA half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. The voltage of the cell is 0.642 V, with the copper as the negative electrode. (a) Write the half-reactions and the overall equation for the spontaneous chemical reaction. (b) Use the standard potential of the copper half-reaction, with the voltage of the cell, to calculate the standard reduction potential for the plutonium half-reaction.arrow_forward
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