What would the potential of a standard hydrogen (S.H.E.) electrode be if it was

Question

          What would the potential of a standard hydrogen (S.H.E.) electrode be if it was under the following conditions?
H+=0.85M, Ph2=4.8 atm, T=298K

THank you!
          What would the potential of a standard hydrogen (S.H.E.) electrode be if it was under the following conditions?
H+=0.85M, Ph2=4.8 atm, T=298K

THank you!
     What would the potential of a standard hydrogen (S.H.E.) electrode be if it was under the following conditions?
H+=0.85M, Ph2=4.8 atm, T=298K

THank you!
What would the potential of a standard hydrogen (S.H.E.) electrode be if it was under the following conditions?
H+=0.85M, Ph2=4.8 atm, T=298K

THank you!

Explanation / Answer

2 H+ + 2 e- => H2

Moles of electrons transferred = n = 2

Faraday constant F = 96485 C/mol

Temperature T = 25 deg C = 298 K

Molar gas constant R = 8.314 J/mol.K

Standard electrode potential Eo = 0.00 V


Nernst equation: E = Eo - RT/nF ln(P(H2)/[H+]^2)

= 0.00 - 8.314 x 298/(2 x 96485) x ln(4.8/0.85^2)

= -0.0243 V = -0.024 V

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