1. Balance the following red-ox equation: MnO4(q)+H2C2O4(aq)Mn(aq)2++CO2(g) Make sure you Identify the oxidation and reduction half reactions, who is the reducing and oxidizing agent and what is the total number of electrons transferred. 2. Use tabulated half-cell potentials to calculate G for the following redox reaction: Pb(aq)2++Cu(s)Pb(s)+Cu(aq)2+ Is it a spontaneous reaction? 3. Determine the redox reaction represented by the following cell notation: Fe(s)Fe(aq)2+Cu(aq)2+Cu(s) 4. The standard emf for the cell using the overall cell reaction below is +0.48V : Zn(s)+Nii(aq)2+Zn(aq)2++Ni(s) What is the emf generated by the cell when [Ni2+]=2.50M and [Zn2+]= 0.50M