multiple choice question In class, we have begun learning about the 2nd Law of T
ID: 555710 • Letter: M
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multiple choice question In class, we have begun learning about the 2nd Law of Thermodynamics which makes a grand statement that "All spontaneous processes increase the entropy of the universe." We then learned about an equation that describes the entropy change of the surroundings as: AS surroundings where the delta H is the enthalpy change (J) of the system and T is Kelvin temperature. We went on to derive an equation for change in Gibbs Free energy (delta G)-which is a crucial variable for us as it serves as a 'chemical potential energy' that allows us to predict whether a reaction will occur at a certain temperature. Why was the above equation crucial for defining the Gibbs free energy change? A. because it allowed us to define delta G in terms of characteristics of the reaction system only B. because the enthalpy of exothermic processes is always a positive number C.Explanation / Answer
option C is correct to an extent
since by the entropy change of the surrounding computation we can compute the entropy changes involved in the system and that will further be used in the computation of change in gibbs free energy.
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