Ag(s) Pb(s) salt bridge True True Determine which of the following statements about the cell shown are True or False. The standard cell potential, o, equals 0.93 V. As the reaction proceeds, the concentration of the silver ions decreases. False Cations move to the lead half-cell. True The mass of the silver electrode is increasing. True The silver half-cell is the cathode. False The cell, as represented by the line notation, is a voltaic cell. True The lead electrode is the anode. True Electrons are spontaneously produced in the silver half-cell. Pb+2 Ag NO So Pb2+20→→ Pb(s) E--0.13V Ag + le → Ag(s) E-+0.80V Pb(s) Pb2+ (1M) || Ag+ (1M) | Ag(s)

4 A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of MSO and the right half cell with a 75.0 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 40.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. left right x10 X Ś

In a electrochemical cell, which of the following statements is true?     In a galvanic cell, the substance at the anode loses electrons but in a electrolytic cell, the substance at the cathode loses electrons.     The substance at the anode loses electrons.     The substance in the salt bridge loses electrons.     The substance at the cathode loses electrons.

Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode.   Cl2        +          Br-       ->         Cl-        +          Br2