Question

an electrochemical cell consists of a silver electrode in contact with 346mL of 0.100 M AgNO3 solution and magnesium electrode wit 288mL of a 0.100 M Mg(NO3)2 solution. (a) What is the emf of the cell? (b) What is the spontaneous cell reaction? (c) a current is drawn from then cell until 1.20g of silver have deposited on the silver electrode. What is the emf for the cell at this stage of the operation? (d) What is the equilibrium constant of the cell reaction?

Answer 1

So lutions Anode MY 2 e Ca tho de AY e Net 2 & tandard cel. a'th OM Fuy gtanda emf 3 (-2.37 an Froduts, ouid uso Nemz E in for mon -Stmda rd call EMF dtenda on conc 3.17- RT ent Ec Eu RI ing Cet - 3.17-(e314)(2) 2 Ca6500) 0-10)2 3.14 V 1 иiner ton yenaning in salution e dosion -20 nener mutal firt we catulati the Ay n ally in rlutión mad AT Аg ditoind :20 mal 07.9 Triin han - (34ivmol A)- mt (3u6x7 mol Ay sluton } x10?m{Ag). A3.351ol O.346 6-74 x10 M

Overall ea uipn is ' can) Mg (s)2 memano balanced, uahon, to ind amoon mual Sutferi oxidartn c (-1 x1o2 mol ) 2 ml x 1mel m M Solution oas Amornt o.28 L YQ.100 mol New Lon conmratin is .- +(2.88 Io New cu mf a :- 0. 0257 V C 3.17 V- em o.119 3-13 Nu Emf = 3.13v