we constructed galvanic cells with the following solutions (with a their respective metals used as cathodes): KNO3 was used to construct a salt bridge to all the following solutions: ZnSO4, CuSO4, FeSO4, NI(NO3)2, KI/I2. we then used a multimeter to test voltaages, this is what we came up with for results: Cell Anode Cathod Voltage Assuming that the reduction potential for the most active metal is 0 V Zn + Cu Zn Cu 1.01 Using observed voltages determine the reduction potentials for the other Zn+Fe Zn Fe .39 oxidized species investigated. Zn+NI Zn Ni .25 what was strongest oxidizing agent?/reducing agent? Zn+I2/I- Zn I2/I- 1.31 what is the highest cell voltage that could be used from the half Fe+Ni Ni Fe .16 cells used in this experiment? Fe + I2/I- Fe I2/I- .92 supposed taht Fe/Fe2+ was used as the reference reaction instead of the one that included the most active metal. what would Ni+I2/I- Ni I2/I- 1.03 the highest cell voltage that could be constructed from 1/2 cells be? determine value for delta G0 for the following systems using your value for E0 Zn + Fe2+ = Zn2+ + Fe Cu + Zn2+ = Cu2+ + Zn order the following in order of activity, w/ most active first: Cu, H, Fe, Ni, Zn, Na, Mg, Ag