b) The following chemical reaction is occurring in an electrochemical cell: Mg) + 2Ag* (0.0001M) ...

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b) The following chemical reaction is occurring in an electrochemical cell: Mg) + 2Ag* (0.0001M) → Mg²*(0.10 M) + 2Ag) The E° electrode value are: Mg²+/Mg= -2.36 V Ag*/Ag = 0.81 V Calculate i. the E° value for the electrode 2Ag"/2Ag. (2) ii. Standard cell potential E°. (2) iii. Will the above cell reaction be spontaneous? Why? (2) iv. Cell potential using Nernst equation. (5) [21] b) The following chemical reaction is occurring in an electrochemical cell: Mg) + 2Ag* (0.0001M) → Mg²*(0.10 M) + 2Ag) The E° electrode value are: Mg²+/Mg= -2.36 V Ag*/Ag = 0.81 V Calculate i. the E° value for the electrode 2Ag"/2Ag. (2) ii. Standard cell potential E°. (2) iii. Will the above cell reaction be spontaneous? Why? (2) iv. Cell potential using Nernst equation. (5) [21]