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user7951
user7951

I'mI’m dealing with electrochemistry problems. For the following reaction $$2H^+ + 2e^- \leftrightarrow H_2 \ \ \ \ \ \ \ E^o= 0 \ V$$$$\ce{2H+ +2e- <=>H2}\quad E^\circ=0\ \mathrm{V}$$ Does it make sense to say $$\Delta G^o=-nFE^o = 0 $$$$\Delta G^\circ=-nFE^\circ=0$$ Which would mean the reaction is in equilibrium?

I'm dealing with electrochemistry problems. For the following reaction $$2H^+ + 2e^- \leftrightarrow H_2 \ \ \ \ \ \ \ E^o= 0 \ V$$ Does it make sense to say $$\Delta G^o=-nFE^o = 0 $$ Which would mean the reaction is in equilibrium?

I’m dealing with electrochemistry problems. For the following reaction $$\ce{2H+ +2e- <=>H2}\quad E^\circ=0\ \mathrm{V}$$ Does it make sense to say $$\Delta G^\circ=-nFE^\circ=0$$ Which would mean the reaction is in equilibrium?

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milo
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Delta G for Standard Hydrogen Electrode reaction

I'm dealing with electrochemistry problems. For the following reaction $$2H^+ + 2e^- \leftrightarrow H_2 \ \ \ \ \ \ \ E^o= 0 \ V$$ Does it make sense to say $$\Delta G^o=-nFE^o = 0 $$ Which would mean the reaction is in equilibrium?