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If the `E_(cell)^(@)` for a given reaction has a positive value, then which of the following gives the correct relationship for the values of `DeltaG^(@)` and `K_(eq)` :-A. `DeltaG^(@)lt0,K_(eq)lt1`B. `DeltaG^(@)gt0,K_(eq)gt1`C. `DeltaG^(@)gt0,K_(eq)lt1`D. `DeltaG^(@)lt0,K_(eq)gt1` |
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Answer» Correct Answer - D `E_(cell)^(@)=positive` `DeltaG^(@)=nF E_(cell)^(@)` `DeltaG^(@)=Negative` `DeltaG^(@)=-2.303RTlogK_(eq)` `"log"K_(eq)=+"ve value"` `K_(eq)gt1` |
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