Wednesday
April 23, 2014

Homework Help: chemistry

Posted by chem help please on Thursday, December 6, 2012 at 5:42pm.

QUESTION: Calculate the standard free-energy change (deltaG°) for the following reaction at 25 °C in kJ.

2Ag^3+(aq) + 3Zn(s)<==> 2Au(s) + 3Zn^2+(aq)


here's what i have so far:
first i wrote out the half reactions:
Au^3+(aq) + 3e^- --> Au(s) = +1.52*2
Zn(s) --> Zn^2+(aq) + 2e^- = +0.76*3

so E°cell= (1.52 * 2) + (0.76 * 3)=5.32V

then i plugged it into the equation..
deltaG°= -nFE°cell, where F=96,485 C/mol

am i on the right track? how do i find n so i can solve for deltaG°?

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