Can someone explain how the change in entropy of a reaction decreases with Increasing temperature?
dS = q/T
I understand how entropy itself increases with increasing temperature but how does the change in entropy decrease with increasing temperature?
If we consider a chemical reaction A --> B for which entropy increaes from reactants to products, increasing temperature would increase the temperature for both sides, but does it increase the entropy of the lower entropy side more than it does for the higher entropy side?
Also shouldnt there be a dependence on whether the reaction is endothermic or exothermic? If its exothermic, then the increase in temperature would push the reaction to the reactants. Woudlnt' this affect the change in entropy?
Thanks guys relaly confused here exam krackers is killing me
dS = q/T
I understand how entropy itself increases with increasing temperature but how does the change in entropy decrease with increasing temperature?
If we consider a chemical reaction A --> B for which entropy increaes from reactants to products, increasing temperature would increase the temperature for both sides, but does it increase the entropy of the lower entropy side more than it does for the higher entropy side?
Also shouldnt there be a dependence on whether the reaction is endothermic or exothermic? If its exothermic, then the increase in temperature would push the reaction to the reactants. Woudlnt' this affect the change in entropy?
Thanks guys relaly confused here exam krackers is killing me