Posted by **flame** on Saturday, November 27, 2010 at 1:09am.

The electrochemical cell described by the cell notation has an Eo of -0.37 V. Calculate the maximum electrical work (kJ) the cell has done if 331.73 g of Cu(s) (Molar Mass - 63.55 g/mol) reacts. Round your answer to 3 significant figures.

Cu(s) l Cu+(aq) ll Sn4+(aq), Sn2+(aq) l Pt(s)

St. Red. Pot. (V)

Cu+/Cu +0.52

Sn4+/Sn2+ +0.15

Faraday's Constant

F = 96485 C

n=2

convert 331g to mole= 5.21

G=-nFE=2(5.21)(96485)(-.37)=372kJ, why do i have to divide it in half to get 186kJ

## Answer this Question

## Related Questions

- chemistry - The electrochemical cell described by the cell notation has an Eo of...
- chemistry - The electrochemical cell described by the cell notation has an Eo ...
- chemistry - The electrochemical cell described by the cell notation has an Eo of...
- chemistry - The electrochemical cell described by the balanced chemical ...
- chemistry - The electrochemical cell described by the cell notation has a ...
- chemistry(check my steps) - The electrochemical cell described by the cell ...
- Chemistry - The voltaic cell described by the cell notation has a standard emf (...
- chemistry - The reaction described by the equation Zn + Hg2Cl2 <--> 2Hg +...
- chemistry - The electrochemical cell described by the cell notation has a ...
- CHEMISTRY - The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1...