When does E Cell (not the standard E cell, but the calculated E cell) equal zero
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When does E Cell (not the standard E cell, but the calculated E cell) equal zero

[From: ] [author: ] [Date: 12-04-21] [Hit: ]
But what I dont understand is why the Ecell on left side of the equation as its written is zero. I know the E(v) for hydrogen is zero, but is this why the Ecell value is zero? Because energy must be supplied at conditions that arent standard? Thanks for the help.-I have a little trouble following the question,......
I'm working on a problem right now: What is the equilibrium constant for the oxidation of copper by H+ for the following reaction: Cu(s) + 2H+(aq) >>> Cu2+(aq) + H2(g). I know the E cell value for the reaction the way it is set up is -.34, so I plug that value into the Nernst equation for the standard value, but why does the E cell value on the other side of the Nernst equation equal zero?

Ecell = Ecell(standard e cell) -((RT)/(vEF))ln(Q)

What I'm trying to find is Q. But what I don't understand is why the Ecell on left side of the equation as it's written is zero. I know the E(v) for hydrogen is zero, but is this why the Ecell value is zero? Because energy must be supplied at conditions that aren't standard? Thanks for the help.

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I have a little trouble following the question, so I'll just make some general comments.

E zero is the voltage when everything is at standard state.

You can calculate the actual E at any set of concentrations by plugging those values into Q.

If the actual E is zero, then you have equilibrium conditions and, instead of Q, you have Keq
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