Consider a reaction where S rxn = -315 J/K and H rxn = -45.6 kJ. Which statement
ID: 952407 • Letter: C
Question
Consider a reaction where S rxn = -315 J/K and H rxn = -45.6 kJ. Which statement is true about the spontaneity of this reaction?
A. This reaction is spontaneous at 25°C, but will become nonspontaneous if the temperature is decreased to -130°C. B. Decreasing the temperature will have no effect on the spontaneity of the reaction. It is nonspontaneous at 25°C and will become even less spontaneous as the temperature decreases. C. This reaction is nonspontaneous at 25°C but will become spontaneous if the temperature is decreased to -130°C. D. This reaction is nonspontaneous at 25°C but will become spontaneous if the temperature is increased to 145°C.Explanation / Answer
use the formula
dG = dH - TdS
if dG got -ve reaction is spontaneous
if dG got +ve reaction is nonspontaneous
my choice is option B
because in the given equation delta H term -ve and delta S term negitive and which is very large value