Fuel cells `:` Fuel cells are galvanic cells in which the chemical energy of fuel cell is directly converted into electrical energy. A type of fuel cell is a hydrogen `-` oxygen fuel cell. It consists of two electrodes made up of two porous graphite impregnated with a catalyst `(` platinum, silver, or metal oxide `).` The electrodes are placed in aqueous solution of `NaOH` . Oxygen and hydrogen are continuously fed into the cell. Hydrogen gets oxidized to `H^(o+)` which is neutralized by `overset(c-)(O)H, i.e.,` anodic reaction.

At cathode, `O_(2)` gets reduced to `overset(c-)(O)H`
Hence, the net reaction is
The overall reaction has
`DeltaH=-285.6 kJ mol^(-1)` and `DeltaG=-237.4 kJ mol^(-1)` at `25^(@)C`
What is the value of `DeltaS^(c-)` for the fuel cell at `25^(@)C`?

Options

A. `-1600 J K^(-1)`
B. `-160 J K^(-1)`
C. `160 J K^(-1)`
D. `1600 J K^(-1)`

Answer

b

Explanation

`DeltaG^(c-)=DeltaH^(c-)-T DeltaS^(c-)`
`implies-237.4=-285.6-298DeltaS^(c-)`
`:. DeltaS^(c-)=-160J K^(-1)`