[offlinedoctor]

For the following question,
'An electrochemical cell consists of a SHE and a copper metal electrode. The standard reduction potentials are: H+/H2 = 0.00 V and Cu2+/Cu = 0.34 V. Find the general voltage in non-standard conditions using the Nernst Equation'

What I did:
i) H2 -> H⁺ + e^-
   Cu²⁺+2e^--> Cu
Therefore:
H2 Cu²⁺-> H⁺ + Cu

Wouldn't Q = H⁺/Cu²⁺,
therefore, the Nernst Equation would be;
E = 0.34 - 0.0591x(log(Q))/2
E = 0.34 - 0.0591x(log(H⁺/Cu²⁺))/2 ?

Most of the answers seem to ignore H+ regardless of standard or nonstandard conditions, instead using:
E = 0.34 - 0.0591x(log(1/Cu²⁺))/2
wouldn't H+ concentration need to be considered  as its in aqueous form?

[Borek]

'An electrochemical cell consists of a SHE and a copper metal electrode. The standard reduction potentials are: H+/H2 = 0.00 V and Cu2+/Cu = 0.34 V. Find the general voltage in non-standard conditions using the Nernst Equation'

Final answer depends on pH, hydrogen pressure, and Cu²⁺ concentration, even just H⁺ and Cu²⁺ are not enough.

Most of the answers seem to ignore H+ regardless of standard or nonstandard conditions, instead using:
E = 0.34 - 0.0591x(log(1/Cu²⁺))/2

This is only potential of the copper concentration half cell, not of the entire cell.