(a) Draw a schematic representation of the galvanic (electrochemical) cell that is described by the following cell notation. Label all the components of the cell that are required to enable the spontaneous transfer of electrons and indicate the direction of electron flow using an arrow. Sn(s)|Sn²+ (aq, 1 mol L-1)||Pb²+ (aq, 0.001 mol L-¹)|Pb(s) Sn²+ (aq) + 2e →→ Sn(s) Pb²+ (aq) + 2e →→ Pb(s) Eº = -0.136 V Eº = -0.126 V (b) Calculate the values for Eºcell, AGⓇ and K at 25 °C for the cell from part (a). Show all steps in your calculation

Pb(s) Determine which of the following statements about the cell shown are True or False. True The standard cell potential, o, equals 0.93 V. True 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 True The lead electrode is the anode. Electrons are spontaneously produced in the silver half-cell. salt bridge Ag(s) Pb+2 So Pb2+2e → Pb(s) AS NO3 E--0.13V Ag + le → Ag(s) E° - +0.80V Pb(s) Pb2+ (1M) || Ag+ (1M) | Ag(s)

Find the nonstandard cell potential for the galvanic cell described by the cell notation provided below. Cr(s)|Cr2+(aq,0.0200M)|| Fe3+(aq,4.00 M)|Fe(s)

The following figure represents an electrochemical cell at 25.00C with aqueous solutions that behave ideally: (a) Represent the electrochemical cell using cell notation, by taking into account that concentrations of the ZnSO4 and CuSO4 solutions are 0.25 M and 0.35 M, respectively. (b) Calculate the standard potential of the cell, E0cell. (c) Calculate the potential of the cell, Ecell. (d)Calculate DG0 (e)Calculate DG (f)Calculate the equilibrium constant, K.