The standard cell potential of this electrochemical cell at 298 K isAnswer with two decimal places, without units.Ni(s) N2+(aq)||Ag+(aq)|Ag(s)Ag (s) + eAg(s)E = 0.80 VNi2+(aq) + 2eNi(s)E = -0.26 VV.

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Chemistry: Matter and Change

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Chapter20: Electrochemistry

Section20.1: Voltaic Cells

Problem 13SSC

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a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
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At 298 K, the solubility product constant for Pb(IO3)2 is 2.6 1013, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction Pb(IO3)2(s)+2ePb(s)+2IO3(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions, and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/Pb(IO3)2 electrode in a 3.5 103 M solution of NaIO3.
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The standard cell potential of this electrochemical cell at 298 K is Answer with two decimal places, without units. Ni(s) N2+(aq)||Ag+(aq)|Ag(s) Ag (s) + e Ag(s) E = 0.80 V Ni2+(aq) + 2e Ni(s) E = -0.26 V V.