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Question
Relationship between equilibrium constant of the reaction and standard electrode potential of electrochemical cell in which that reaction takes place is ____________.
Options
`"E"_"cell"^0 = (2.303 "RT")/("nF") log "K"_"c"`
`"E"_"cell"^0 = (2.303 "RT")/("F") log "K"_"c"`
`"E"_"cell"^0 = (2.03 "RT")/("nF") log "K"_"c"`
`"E"_"cell"^0 = (2.230 "RT")/("nF") log "K"_"c"`
MCQ
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Solution
Relationship between equilibrium constant of the reaction and standard electrode potential of electrochemical cell in which that reaction takes place is `underline("E"_"cell"^0 = (2.303 "RT")/("nF") log "K"_"c")`.
Explanation:
∆G0 = − 2.303 RT log Kc; ∆G0 = `-"nFE"_"cell"^0`
Equating, `"E"_"cell"^0 = (2.303 "RT")/"nF" log "K"_"c"`
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