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A student places a zinc electrode in a 0.80 M Zn2+(aq) solution which is connected by anelectrolyte to a 1.30 M Ag+(aq) solution
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1) Using a table of standard electrode potentials (such as the one in your textbook), calculate thestandard cell potential for a
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1) Using a table of standard electrode potentials (such as the one in your textbook), calculate thestandard cell potential for a
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Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a
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and i leave Zn's positive right? or do i change it back to negative now?
Oh duh ok i get that thanks a million
never mind you are right with the log part so i just don't understand what n is
what is n? and isnt it ln not log? so Ecell=1.56-(.0592/n)ln(.76/.80)?
reduction potential for the Zn is -.76 for Ag it is .80 so i take the Zn change the sign so it it .76 then i go .76+.80=1.56 does this sound right?

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