What are E and AG of a redox reaction at 25°C for which n= 2 and K= 0.075? cell E cell V AG°- %3D J

Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4H+ Fe3+ + e-= Fe²+ E° = 0.771 V 0, + 2 H* + 2 e¯2 H,0 E° = 1.229 V E° = V K = Is the overall reaction spontaneous as written? AG° = spontaneous not spontaneous

For the galvanic cell at 298 K 2X(s) + 3Y2*(aq) –→ 2x3*(aq) + 3Y(s) E° cell = 0.39 V What is the measured cell potential (Ecell) when [Y2*] = 1.0 M and [X3+] = 0.01 M? Periodic Table and Datasheet O 0.39 V O 0.35 V O 0.43 V O 0.51 V

Standard Reduction Potentials (Volts) at 25 °C F2 (g) + 2 e-  2 F- (aq) 2.870 O2(g) + 4 H3O+(aq) + 4 e-  6 H2O(l)  1.229 2 H2O(l) + 2 e-  H2(g) + 2 OH-(aq) -0.828 Fe2+ (aq) + 2 e-  Fe (s) -0.440   A 0.122 M neutral aqueous FeF2 solution is electrolyzed under 1 atm pressure using platinum electrodes.(a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials.Half-reaction at anode:     +       +       ->       +       +     Half-reaction at cathode:     +       +       ->       +       +     (b) What is the expected decomposition potential? _______ V

The free energy change for the following reaction at 25 °C, when [Cu2+] = 2.57x10-³ M and [I₂] = 1.10 M, is 88.8 kJ: 2Cu²+(2.57x10-3 M) + 2.001 (aq)—2Cu+ (aq) + 1₂(1.10 M) AG= 88.8 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?

Calculate the theoretical cell potential for the following galvanic cell: Mg | Mg2+ ( 1 M) || Cu2+ (2 M) | Cu

Which of the following reactions occurs at the anode of an electrochemical cell composed of Zn│Zn2+(aq) and Fe│Fe2+(aq) half-cells? Their reduction potentials are as follows:                 Zn2+   +  2e–   -->  Zn;    Eo = -0.763 V                              Fe2+  +  2e–   -->  Fe;      Eo = -0.447 V     (A) Zn2+ + 2e– -->  Cr;                     (B) Zn -->  Zn2+ + 2e–;                    (C) Fe -->  Fe2+ + 2e–;              (D) Fe2+ + 2e– -->  Fe;