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b) The following chemical reaction is occurring in an electrochemical cell: Mg) + 2Ag* (0.0001M) Mg*(0.10 M) + 2Ag) The E electrode value are:
b) The following chemical reaction is occurring in an electrochemical cell: Mg) + 2Ag* (0.0001M) Mg*(0.10 M) + 2Ag) The E electrode value are: Mg+/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]
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General Chemistry
Authors: Darrell Ebbing, Steven D. Gammon
9th edition
978-0618857487, 618857486, 143904399X , 978-1439043998
