The following electrochemical data may be helpful in answering the question below. Use the table of Standard Reduction Potentials. Calculate the ΔGo for the oxidation of silver according to the following balanced reaction. 2Ag(s) + CaI2(aq)  Ca(s) + 2AgI(s)

Complete and balance the following redox reaction in basic solution. ReO4-(aq)+Pb2+(aq) = Re(s)+PbO2(s)

Balance the following redox equation to its lowest integer ratio. (Under Acidic Conditions) Te(s)    +    Ru(NO3)3(aq)  +   NO2(g)   ↔   Ru2Te3(s)  +   HNO3(aq)   Note that H2O and H+ are not shown in the equation above.  If it is required to balance the equation, then add these.Fill in the coefficient for each chemical after you finish balancing the equation.  If the chemical is not needed in the equation then mark a zero next to it    Te(s)   HNO3(aq)  H2O(l)  Ru2Te3(s)   NO2(g)   Ru(NO3)3(aq)   H+ (aq)

Use the standard reduction potentials located in the Tables' linked above to calculate the standard free energy change in kj for the reaction: Fe²+ (aq) + Hg(1)→ Fe(s) + Hg²+ (aq) Answer: 237.16 K for this reaction would be greater than one.

Suppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 A£NO3(aq) → Cu(NO,),(aq)+2 Ag(s) E1 E2 sí S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. O-0 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? O DD

If a 6.0 Amp current is used, calculate the number of hours needed to prepare 22.0 grams of calcium metal from calcium ion. The reduction potential is -2.39 V

Calculate the voltage of the redox reaction of element X (group 2) if the Gibb’s free energy evolved during the redox reaction is + 150 kJ/mol. (Faraday constant, 9.649 x 104C)