For the electrochemical cell described, what is the value of E when [Ni²+] = 0.53 M? Assume T is 298 K. Ni(s) + Sn2+(aq) → Ni²+(aq) + Sn(s) (E° = 0.120 V, [Sn²+] = 1.75 M)
For the electrochemical cell described, what is the value of E when [Ni²+] = 0.53 M? Assume T is 298 K. Ni(s) + Sn2+(aq) → Ni²+(aq) + Sn(s) (E° = 0.120 V, [Sn²+] = 1.75 M)
Chemistry: Principles and Reactions
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Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter17: Electrochemistry
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![For the electrochemical cell described, what is the value of E when [Ni²+]
= 0.53 M? Assume T is 298 K.
Ni(s) + Sn2+(aq) → Ni²+(aq) + Sn(s) (E° = 0.120 V, [Sn²+] = 1.75 M)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F627ffe10-a730-4e4c-b7e9-b306478e5985%2F8a18aaed-4e83-4b5b-88da-54a5cfc71fb7%2Fb4urh7e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:For the electrochemical cell described, what is the value of E when [Ni²+]
= 0.53 M? Assume T is 298 K.
Ni(s) + Sn2+(aq) → Ni²+(aq) + Sn(s) (E° = 0.120 V, [Sn²+] = 1.75 M)
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