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3 July, 09:26

What would the potential of a standard hydrogen electrode (s. h. e.) be under the given conditions? [h+]=0.70 mph2=2.4 atmt=298 k?

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  1. 3 July, 09:49
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    Constant = 8.314JK⁻¹mol⁻¹

    T is for temperature which is 298K

    Faraday constant value is 96500C/mol

    n is the number of electrons which are transferred in the reaction.

    Ecell = E₀cell - RT/nFiN [cathode]/[anode]

    Ecell = E₀cell - RT/nF In [PH₂]/[H⁺]²

    Ecell = 0.00-8.314 JK⁻¹ mol⁻¹ * 298k / 2 * 96500C/mol In [2.4atm] / 0.70]²

    Ecell = 0.00 - 0.0129 In (2.59)

    Ecell = 0.00 - 0.0129 * 0.951

    Ecell = - 0.0122V

    ∴Ecell is = - o. 0122v
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