Designing a galvanic cell from two half-reactions chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2103(aq)+12 H(aq)+10e →>> - I2(s)+6H2O(l) Br₂(1)+2e → 2 Br (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that ☐ happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. ☐ Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. ☐ Do you have enough Yes information to calculate the cell voltage under standard No conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer V Eº red Eº 'red = +1.195 V = +1.065 V ☑ ☐ x10 ك

Designing a galvanic cell from two half-reactions chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2103(aq)+12 H(aq)+10e →>> - I2(s)+6H2O(l) Br₂(1)+2e → 2 Br (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that ☐ happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. ☐ Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. ☐ Do you have enough Yes information to calculate the cell voltage under standard No conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer V Eº red Eº 'red = +1.195 V = +1.065 V ☑ ☐ x10 ك

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.49QE: A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt...

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An 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?
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)
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
What 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)?
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
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).
Consider 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?
A 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.
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .