The standard potential of a cell using the reaction is `1.12`. The heat of the reaction is `-504.2kJ mol ^(-1)` at `25^(@)C`. Calculate the entropy change.

The standard potential of a cell using the reaction is `1.12`. The he

1.	The standard potential of a cell using the reaction is `1.12`. The heat of the reaction is `-504.2kJ mol ^(-1)` at `25^(@)C`. Calculate the entropy change.
Answer» `2Ni(s)+4H_(2)Orarr 2Ni(OH)_(2)+4H^(o+)+4e^(-)` `4H^(o+)+O_(2)+4e^(-)rarr2H_(2)O` `DeltaG^(c-)=-nFE^(c-)=-4xx96500xx1.12=-432320J` `DeltaG^(c-)=DeltaH^(c-)-TDeltaS^(c-)` `:. DeltaS^(c-)=(DeltaH^(c-)-DeltaG^(c-))/(T)` `=-(504.2xx10^(3)J-(-432320))/(298)` `=-241.2JK^(-1)mol^(-1)`

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The standard potential of a cell using the reaction is `1.12`. The heat of the reaction is `-504.2kJ mol ^(-1)` at `25^(@)C`. Calculate the entropy change.

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