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Write the Nernst equation and emf of the...

Write the Nernst equation and emf of the following cells at 298K.
(i) `Sn(s) | Sn^(2+) ( 0.050M)|| H^(+) ( 0.020M)| H_(2) ( g, 1"bar") | Pt(s)`
(ii) `Pt(s) | Br_(2) ( l ) | Br^(-)(0.010M) || H^(+) (0.030M) | H_(2)(g, 1"bar") | Pt (s)`

Answer

Step by step text solution for Write the Nernst equation and emf of the following cells at 298K. (i) Sn(s) | Sn^(2+) ( 0.050M)|| H^(+) ( 0.020M)| H_(2) ( g, 1"bar") | Pt(s) (ii) Pt(s) | Br_(2) ( l ) | Br^(-)(0.010M) || H^(+) (0.030M) | H_(2)(g, 1"bar") | Pt (s) by CHEMISTRY experts to help you in doubts & scoring excellent marks in Class 12 exams.

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Write the Nernst equation and emf of the following cell at 298K. Fe(s) | Fe^(2+) ( 0.001M) || H^(+) ( 1M ) | H_(2) ( g) ( 1"bar") | Pt .

Write the Nernst equation and emf of the following cell at 298 K. (i) Mg(s) |Mg^(2+) ( 0.001 M) || Cu^(2+) ( 0.0001M ) | Cu(s) (ii) Fe(s) | Fe^(2+) ( 0.001M) || H^(+) ( 1M) | H_(2)(g) (1 "bar") | Pt(s) Given that, E_(Mg^(2+) //Mg)^(@) = - 2.36V , E_(Cu^(2+) Cu)^(@) = 0.34V, E_(Fe^(2+)Fe)^(@) = -0.44V

Knowledge Check

  • The cell reaction for the given cell is spontaneous if : Pt | Cl_2|CI^(-) (1M)||CI^(-) (1M)|Cl_2| Pt

    A
    `P_1 gt P_2`
    B
    `P_1 lt P_2`
    C
    `P_1=P_2`
    D
    `P_2=1` atm

  • The potential of the following cell is 0.34 V at 25^(@)V . Calculate the standard reduction potential of the copper half-cell . Pt| H_(2) ( 1 atm) | H^(+) ( 1M) || Cu^(2+) ( 1M) | Cu

    A
    `-3.4 V`
    B
    `+3.4V`
    C
    `- 0.34V`
    D
    `+0.34V`

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