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25. The reduction potentials for Au3* and Ni2* are as follows: R Aur* + 3e- -+ Au E" : +1.50 V n Ni2* + 2e- -+ Ni E :4.23 Y U- Calculate AGo (at 25'C) for t}re reaction: 2Au3* + 3Ni-+ 3Ni2* + 2Au b a)-2l40kJ b) +5.00 x 102 kJ @t.oo x lo3 kJ d) +1.00 x l0'kJ e) -5.00 x 102 kJ t = t.\-L'o't)) + t.Jz",t. D0" = -nFE"rd), Qlc)-v : *br lbut5x ,-tl P'K-Tfr"c 26. Determine the equilibrium constant at2ioC for the reaction t-- Zn + Ni?+ -+ Zn2+ + Ni Zn?+ + 2e- -+@ r@+2e-+ Ni a)4.1 x 103 b) 9.3 x 108 c) 6.4 x l0{ @-o
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Unformatted text preview: " r^o'-' e) none ol these-o-rt -Gt'1b) = o'J] v 27. A concentration cell is constructed using two$! electrodes with Niz* concentrations of 1.0 M and 1.00 x l0{ M iq the two half-cells. The reduction potential ofNi2* is -{.23 V. Calculate the potential of the cell at25"C. trSo.r ra v Yl.ifl} ,' 'i-l Ni't t :e *> ui Ed= -e'>3 V Q-o-" d) +0.132 v e) +0.0592 V = Jr{ ,9 ul /N. Y: -0.76v e,t^= E:4.23Y lnq k= ln Eo \., oofl I o'o}? 'q?E -+ f = €" -= =zz1 o. 6...
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This note was uploaded on 12/27/2011 for the course CHEM 122 taught by Professor Williams during the Fall '10 term at Simon Fraser.

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