Final answer:
The change in enthalpy of the surroundings (∆H-surroundings) is inversely related to the change in enthalpy of the system (∆H-system) in an isobaric and isothermal process, and is associated with the entropy change of the surroundings (∆S-surroundings) as calculated by ∆S-surroundings = -∆H-system/T.
Step-by-step explanation:
In an isobaric (constant pressure) and isothermal (constant temperature) process, the change in enthalpy (∆H) of the surroundings is directly related to the change in enthalpy of the system. During a chemical reaction, heat is transferred between the system and its surroundings. If the reaction is exothermic (releases heat), the surroundings will get warmer, and ∆H-system will be negative. Conversely, for an endothermic reaction (absorbs heat), the surroundings will get cooler, and ∆H-system will be positive. Using the thermodynamic definition of entropy (S), the change in entropy of the surroundings (∆S-surr) can be determined by the heat flow (qp) accompanied by the reaction and the temperature (T) of the surroundings. This relationship is represented by the equation ∆S-surr = -∆H-system/T, which indicates that for a spontaneous reaction, the total entropy change of the universe (∆S-univ) must be greater than 0.