A voltaic cell consists of a standard hydrogen electrode and a second half-cell in which a magnesium electrode is immersed in a 1.00 M solut

Question

A voltaic cell consists of a standard hydrogen electrode and a second half-cell in which a magnesium electrode is immersed in a 1.00 M solution of Mg2+ ions. Calculate Ecell given that the standard reduction potential for the magnesium half-reaction is -2.37 V.

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Linh Đan 3 mins 2021-07-22T20:15:47+00:00 1 Answers 0 views 0

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    2021-07-22T20:16:47+00:00

    Answer:

    The correct answer is “+2.37 V“.

    Explanation:

    Given that,

    Concentration of Mg^{2+}

    = 1.00 M

    E^0 \ Mg^{2+}/Mg,

    = -2.37 V

    E^0 \ \mu^+/H_2,

    = 0.00V

    When S.H.E as well as anode act as cathode, then

    E^0 cell=E^cathode-E^0 anode

    By putting the values, we get

    ⇒            =0.00V-(-2.37 V)

    ⇒            =+2.37 \ V    

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