Homework Answers
Del G is the change in Gibb's free energy of a chenical reaction at any given condition of temperatures and pressure.
Whereas del G° is the change in gibbs free enegy only at the standard condition i.e at temperature 298 K and pressure 1 atm
Now spontaneity of a reaction is determined as per del G°.
If delG° is positive then the reaction is not spontaneous where as if delG° is negative the reaction is spontaneous.
Now to find the equilibrium constant (K) we use the value of delG° and not delG
i.e delG° = -RT lnK
Where R = gas constant
And T = given temperature in Kelvin
So the correct statements are-
1- A reaction where delG° is positive can never be spontaneous
3- delG is true under any condition
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