AP Chemistryhardmcq1 pt
Given ΔH = -92 kJ and ΔS = -199 J/K for a reaction, it will be spontaneous at:
A.No temperature
B.Temperatures below 462 K
C.Temperatures above 462 K
D.All temperatures
Explanation
Core Concept
ΔG = ΔH - TΔS. For spontaneity, ΔG < 0: -92000 - T(-199) < 0, so T(-199) < -92000, T > 462 K. But ΔS is negative, so high T makes ΔG positive. The reaction is only spontaneous when T < 462 K.
Correct Answer
BTemperatures below 462 K
Practice more AP Chemistry questions with AI-powered explanations
Practice Unit 6: Thermodynamics Questions →