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?

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