The deltaS for a reaction is 3.0 J/(mol*K) at 25 degrees C. Caluculate the deltaG for the reaction when DeltaH = -394 kL and determine whether it will occur spontaneously at this temperature

Answer 1

delta G = delta H -T*deltaS
You must mean -394 kJ and not kL for DH.
What's the problem is just plugging in and getting the answer? The USUAL problem with students is they forget DH is in kJ and DS is in J.
So you want -394 kJ -(298.15)*.003 = ?? kJ.
If the sign is negative, the reaction is spontaneous. If +, the reaction is not spontaneous.

Answer 2

so would it be -2.0764 or do i need to move the decimal?

Answer 3

I don't know how you obtained -2.0764.
-394-(298.15*-0.003) = -394-0.894 = ??.
I changed 3 J/mol*K to kJ/mol*K.