Electrochemical Cells

Cell potential is the measure of the voltage difference between the anode and cathode.
$%5CDelta%20G%20%5C%2C%20of%20%5C%2C%20H_2O(l)%3D-237.2%20KJ%2Fmol$
$%5CDelta%20G%20%5C%2C%20of%20%5C%2C%20CO_2(g)%3D-394.4%20%5C%2C%20KJ%2Fmol$
$%5CDelta%20G%20%5C%2C%20of%20%5C%2C%20pentane%20(g)%3D-8.2%20kJ%2Fmol$

In pentane-oxygen fuel cell following reaction takes place

$C_5H_%7B12%7D%2B10H_2O(l)%20%5Crightarrow5CO_2%2B32%20H%5E%2B%20%5C%2C%20%2B32e%5E-$

$%5Cfrac%20%7B8O_2%2B32H%5E%2B%5C%2C%20%2B32e%5E-%20%5Crightarrow%2016H_2O(l)%7D%20%7BC_5H_%7B12%7D%2B8O_2%20%5Crightarrow5CO%5E2%2B6H_2O(l)%2C%20E%5E0%3D%3F%20%7D$

$%5CDelta%20G_%7Breaction%7D%3D%5Cboldsymbol%7B%5CSigma%7D%20%5CDelta%20G_%7Bproduct%7D-%5Cboldsymbol%7B%5CSigma%7D%20%5CDelta%20G_%7Breactant%7D$
$%3D5%20%5Ctimes%20%5CDelta%20G_%7B(CO_2)%7D%2B6%5CDelta%20G_%7B(H_2O)%7D-%5B%5CDelta%20G_%7B(C_5H_%7B12%7D)%7D%2B8%20%5Ctimes%20%5CDelta%20G_%7BO_2%7D%5D$
$%3D5%20%5Ctimes%20(-394.4)%2B6%20%5Ctimes%20(-237.2)-(-8.2%20%2B0)$
= - 1972- 1423.2+ 8.2
= -3 3 8 7 kJ/mol
$%5C%2C%20%5C%2C%20%5C%2C%20%5C%2C%20%5C%2C%20%5C%2C%20%5C%2C%20%5C%2C%20%3D-3387%20%5Ctimes%2010%5E3%20J%2Fmol$

$%5CDelta%20G%3D-nFE%5E0_%7Bcell%7D$

$-3387%20%5Ctimes%2010%5E3%3D-32%20%5Ctimes%2096500%20%5Ctimes%20E%5E0_%7Bcell%7D$

$%5C%2C%20%5C%2C%20%5C%2C%20%5C%2C%20%5C%2C%20E%5E0_%7Bcell%7D%3D%20%5Cfrac%20%7B-3387%20%5Ctimes%2010%5E3%7D%7B-32%20%5Ctimes%2096500%7D%3D1.0968%20V$

High-Yield Trend

Chapter Questions
1 MCQs

Official Solution

Electrochemical Cells

High-Yield Trend

Chapter Questions 1 MCQs

Official Solution

Chapter Questions
1 MCQs