Question

a) Part a. Define A, Z, and X in the following notation used to specify a nuclide: A 2X. Part b. How are A and Z related? Part c. How many protons and how many neutrons are there in the common radiotracer, Iron-59? b) For the following redox reaction at 25°C, Ecell = 2.24 V. Calculate the equilibrium constant, K. Mg(s) + Pb 2+ (aq) + Mg - (aq) + Pb(s) c) A voltaic cell is set up with one beaker containing 1.0 M Cu(NO :) 2 and a copper electrode, and another beaker containing 1.0 M Mn(NO 3) 2 and a manganese electrode. Given the following standard reduction potentials, answer the 3 questions below: E 10.34 V Cu2+(ag) + 2e → Cu(s) Mn-(aq) + 2e → Mn(s) |-1.18V Part a. Write out the half-cell reaction that occurs at the anode of the voltaic cell. Part b. In which direction do electrons flow? Part c. What is the Eºceu? (Show your work.) d) A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) → Cu 2+ (aq) + 2 Ag(s) The Eºcell for the reaction is +0.46 V. The initial (nonstandard) conditions are: (Ag +) = 2.0 M; [Cu 2+] = 0.025 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is the cell potential, E cell under the non-standard initial conditions?