(2) What Zinc ion concentration is necessary for the actual cell potential to be (a) 0.250 volts, (b) 0.200 volts? Presume all other variables are at standard conditions. Zn + Cr" Cr + Zn²+

Calculate ΔG° for the redox reaction represented by the cell diagram       Pt(s) | Cl2(g, 1 atm)  || ZnCl2(aq, 1 M) | Zn(s).

Consider the following galvanic cell: Cu(s) | Cu²+ (aq) || Ag+(aq) | Ag(s) Identify the cathode and state if it is being oxidized or reduced (please refer to chart on reference data page.) (A) Cu is the cathode; it is being oxidized (B) Cu is the cathode; it is being reduced (C) Ag is the cathode; it is being oxidized (D) Ag is the cathode; it is being reduced (E) Since the E values for both Ag and Cu are positive, they are both cathodes and being reduced

3. At 298 K, the EMF of the cell shown below is +0.84 V. Pt(s)|Fe²*(aq, a = 1), Fe³*(aq, 1)|| Ce**(aq, a = 1), Ce³*(aq, a = 1)|Pt(s) a = (i) Define what is meant by the standard EMF of the cell. (ii) Write down the cell reaction and the Nernst equation for the cell. (iii) Calculate the equilibrium constant for the cell reaction at 298 K.