Question
Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation
ΔG∘=−nFE∘
where n is the number of moles of electrons transferred and F=96,500C/(mol e−) is the Faraday constant. When E∘ is measured in volts, ΔG∘ must be in joules since 1 J=1 C⋅V.
Calculate the standard free-energy change at 25 ∘C for the following reaction:
Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
Express your answer to three significant figures and include the appropriate units.
I thought it was 373 kj*mol^-1 buts its saying something is wrong
ΔG∘=−nFE∘
where n is the number of moles of electrons transferred and F=96,500C/(mol e−) is the Faraday constant. When E∘ is measured in volts, ΔG∘ must be in joules since 1 J=1 C⋅V.
Calculate the standard free-energy change at 25 ∘C for the following reaction:
Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
Express your answer to three significant figures and include the appropriate units.
I thought it was 373 kj*mol^-1 buts its saying something is wrong
Answers
DrBob222
If you will show what you did perhaps we can find the problem. Other than guessing, however, we don't know what you've done.