Question

Using standard potentials given in the appendices, calculate the standard cell potentials for the following reaction: Cu(s) +2Ag (aq)Cu2+ 2Ag(s) Report the answer in volts with three significant figures 0.442 Previous Answers Request Answer Submit X Incorrect; Try Again; 3 attempts remaining Review your calculations; you may have made a rounding error or used the wrong number of significant figures. Part B Determine the equilibrium constant for the above reaction Report to 1 significant figure and using scientific notation 9.1014

Answer 1

E_Ag +^0/Ag = 0.80 v E_cu + 2^0/cu = 0.34 v E_CEU^0 = E_CATHODE^0 - E_ANODE^0 = 0.80 - .34 E_CEU^0 = 0.46 v REDUCTION OCCURS AR CTAHODE OXIDATION OCCURS AT ANODE delta G^0 = -nF E_CEU^0 = -RT ln k n = 2, No. of ELECTRONS TRANSFREED IN THE REACTION T = 298 k, F = 96485 c/mol (FARAORY COSNTANT) ln k = nFE_CEU^0/RT = 2 times 96485 c mol^-1 times 0.46 v/8.314 Jk^-1 mol^-1 times 298 k ln k = 35.83 implies k = e^35.83 EQUILINRUM CONSTANT k = 3.64 times 10^15 (1 CPULOMB - VOLT = 1 JOULE)