5 1/1 point Select all correct statements. A Voltaic cell requires a spontaneous chemical reaction. In an electrochemical cell, the salt bridge provides counterions to correct the charge imbalance caused by the movement of electrons. Electron flows from cathode to anode A possible reaction occurring at the anode of a Voltaic cell is Fe3+ +3e Fe

Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?

Consider a voltaic cell in which the following reaction takes place. 2F2+(aq)+H2O2(aq)+2H+(aq)2Fe3+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Calculate E at 25°C under the following conditions: [Fe2+]=0.00813M,[H2O2]=0.914M,[Fe3+]=0.199M,ph=2.88 .

Give the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?

Consider a voltaic cell at 25°C in which the following reaction takes place. 3H2O2(aq)+6H+(aq)+2Au(s)2Au3+(aq)+6H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Calculate E when [Au3+]=0.250M,[H+]=1.25M,[H2O2]=1.50M .

The half-cells Fe2+(aq) | Fe(s) and O2(g) | H2O (in and solution) 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.

Two Ag+(aq) | Ag(s) half-cells are constructed. The first has [Ag+] = 1.0 M, the second has [Ag+] = 1.0 105 M. When linked together with a salt bridge and external circuit, a cell potential is observed. (This kind of voltaic cell is referred to as a concentration cell.) (a) Draw a picture of this cell, labeling all components. Indicate the cathode and the anode, and indicate in which direction electrons flow in the external circuit. (b) Calculate the cell potential at 298 K.

Balance the following reactions and write the reactions using cell notation. Ignore any inert electrodes, as they are never part of the half-reactions. (a) Al(s)+Zr4+(aq)Al3+(aq)+Zr(s) (b) Ag+(aq)+No(g)Ag(s)+NO3(aq) (acidic solution). (C) SiO32(aq)+Mg(s)Si(s)+Mg(OH)2(s) (basic solution). (d) CIO3(aq)+MnO2(s)CI(aq)+MnO4(aq) (basic solution)

Consider a voltaic cell at 25°C in which the following reaction takes place: MnO2(s)+4H+(aq)+2Br(aq)Br2(l)+Mn2+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Find E under the following conditions: [Mn2+]=0.60M,[Br]=0.83M,pH=3.71 .

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.