Under standard conditions, the ΔGo of the reactants for a given redox reaction is measured to be 211.5 kJ and the ΔGo of products is measured to be 140.3 kJ. If 4 moles of electrons are required in the balanced redox reaction, calculate the standard cell potential, Eocell, for the reaction described here at 25 oC.

You make a voltaic cell with copper and aluminum. If the cell potential is measured to be +2.50 V at room temperature, then what is the reaction quotient?

6) Calculate the potential of a cell, Eºcell, made with a standard bromine electrode as the anode and a standard chlorine electrode as the cathode. Write the shorthand cell notation.

Calculate the cell potential of a cell composed of a cathode consisting of a Co wire immersed in a 1.44 M Co²+ solution and an anode consisting of a Co wire immersed in a 5.60×10-5 M Co²+ solution. Assume the temperature of the solutions is 298 K. Cell potential: V

Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode.   NO3-     +      H+        +      Zn        ->         Zn2+     +       NO2     +       H2O

Determine the cell potential (in volts) of a standard galvanic cell constructed using iron and lead metals and their associated solutions, 1M FeSO4 and 1M PbSO4.

Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+ (aq) and a cathode where Cr3+ (aq) is reduced to Cr2+ (aq) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L and gases have a pressure of 1 bar.

Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode.   MnO4-  +     H+    +      Ce3+     ->         Ce4+     +     Mn2+    +      H2O

Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg? +] = 0.788 M and [Fe² +] = 0.0200 M. Use the standard reduction potentials in this table. Mg(s) + Fe2+(aq) = Mg2+(aq) + Fe(s) E = V

Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. Identify the reactions with K > 1 among the following redox reactions. Write the line representations for the Galvanic cells, indicating the anode and 1. cathode. a. Cl2 + Br → Ct + Br2 b. Mnoa + H* + Ce → Cet + Mn2 + H20