A galvanic cell is set up with iron and aluminum half-cells, according to the unbalanced reaction below. If the concentration of Fe2+ is 0.77 M and the concentration of Al3+ is 0.0011 M, what is the Ecell in volts? Fe2+ (aq) + Al(s)→→ Fe(s) + Al³+ (aq) E cell = +1.22 V OA 1.28 V OB. 1.22 V OC 1.39 V OD. 0.00 V OE. 0.964 V OF 1.13 V OG.1.20 V OH.1.23 V OL 1.05 V 1.33 V

A galvanic cell is set up with iron and aluminum half-cells, according to the unbalanced reaction below. If the concentration of Fe2+ is 0.77 M and the concentration of Al3+ is 0.0011 M, what is the Ecell in volts? Fe2+ (aq) + Al(s)→→ Fe(s) + Al³+ (aq) E cell = +1.22 V OA 1.28 V OB. 1.22 V OC 1.39 V OD. 0.00 V OE. 0.964 V OF 1.13 V OG.1.20 V OH.1.23 V OL 1.05 V 1.33 V

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 48QRT: Consider a voltaic cell with the reaction H2(g) + Sn4+(aq) 2 H+(aq) + Sn2+(aq) operating at 298 K....

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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?
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)
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.
The following oxidationreduction reactions are used in electrochemical cells. Write them using cell notation. (a) 2Ag+(aq)(0.50M)+Ni(s)2Ag(s)+Ni2+(aq)(0.20M) (b) Cu(s)+PtCl62-(aq)(0.10M)Cu2+(aq)(0.20M)+PtCl42-(aq)(0.10M)+2Cl(aq)(0.40M) (c) Pb(s)+SO42-(aq)(0.30M)+2AgCl(s)PbSO4(s)+2Ag(s)+2Cl(aq)(0.20M) (d) In a galvanic cell, one half-cell contains 0.010 M HCI and a platinum electrode, over which H2 is bubbled at a pressure of 1.0 atm. The other half-cell is composed of a zinc electrode in a 0.125 M solution of Zn(NO3)2.
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.
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)
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.
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
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+.
You 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.
Consider a voltaic cell with the reaction H2(g) + Sn4+(aq) 2 H+(aq) + Sn2+(aq) operating at 298 K. (a) Calculate the Ecell for this cell. (b) Calculate the Ecell for PH2 = 1.0 bar, (cone. Sn2+) = 6.0 104M, (cone. Sn4+) = 5.0 104M, and pH = 3.60.