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CET Karnataka Engineering CET - Karnataka Engineering Solved Paper-2009

  • question_answer
    The standard electrode potential for the half cell reactions are                 \[Z{{n}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Zn;\,{{E}^{o}}=-0.76\,V\]                 \[F{{e}^{2+}}+2{{e}^{-}}\xrightarrow{{}}Fe;\,{{E}^{o}}=-0.44\,V\] The emf of the cell reaction,                 \[F{{e}^{2+}}+Zn\xrightarrow{{}}Z{{n}^{2+}}+Fe\] is

    A)  -0.32V                                 

    B)  -1.20V

    C)  + 1.20V                               

    D)  4-0.32 V

    Correct Answer: D

    Solution :

    \[Z{{n}^{2+}}+2{{e}^{-}}\xrightarrow{{}}\,\,Zn;\,\,{{E}^{o}}=-0.76\,V\] \[F{{e}^{2+}}+2{{e}^{-}}\xrightarrow{{}}\,\,Fe;{{E}^{o}}=-0.44\,V\] Cell reaction is                 \[F{{e}^{2+}}\,\,+\,\,Zn\xrightarrow{{}}Z{{n}^{2+}}\,+\,Fe\]                    \[{{E}_{cell}}={{E}_{cathode}}-{{E}_{anode}}\]                 \[=-0.44-\text{(}-0.76\text{)}\]                 \[=-0.44+0.76\]                 \[=0.32\text{ }V\]


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