Redox Reactions And Electrochemistry Ques 597
Question: If the $ E{{{}^\circ } _{cell}} $ for a given reaction has a negative value, then which of the following gives the correct relationships for the values of $ \Delta G{}^\circ $ and $ K _{eq} $ -
Options:
A) $ \Delta G{}^\circ >0;K_{eq}>1 $
B) $ \Delta G{}^\circ <0;K_{eq}>1 $
C) $ \Delta G{}^\circ <0;K_{eq}<1 $
D) $ \Delta G{}^\circ >0;K_{eq}<1 $
Show Answer
Answer:
Correct Answer: D
Solution:
[d] Standard Gibbs free energy is given as $ \Delta G{}^\circ =-nE{}^\circ F $ If $ E{{{}^\circ } _{cell}}<0,i.e.-ve $ $ \Delta G{}^\circ >0 $ Further $ \Delta G{}^\circ =-RT\ell n,K _{eq} $
