Question textAspirin (C9H8O4) is susceptible to degradation by hydrolysis if exposed to water, forming salicylic acid (C7H6O3) and acetic acid (CH3COOH): C9H8O4 (s) + H2O (l) → C7H6O3 (s) + CH3COOH (l) Given the following enthalpies of formation, calculate the enthalpy of the above hydrolysis process per mole of aspirin. State whether the hydrolysis is endothermic or exothermic, justifying your choice from the options available. ∆H°f[C9H8O4 (s)] = −736.4 kJ mol-1 ∆H°f[H2O (l)] = −285.8 kJ mol-1 ∆H°f[C7H6O3 (s)] = −588.4 kJ mol-1 ∆H°f[CH3COOH (l)] = −484.1 kJ mol-1 The enthalpy of hydrolysis is Answer 1 Question 9[input] kJ mol-1 and the hydrolysis is Answer 2 Question 9[select: , exothermic, endothermic] because Answer 3 Question 9[select: , the total number of moles of gas does not change, heat is absorbed from the surroundings during the formation of each of the reactants and products, heat is released to the surroundings during the formation of each of the reactants and products, the system absorbs heat from the surroundings during the hydrolysis, the system releases heat to the surroundings during the hydrolysis, the entropy change during the hydrolysis is negligible]多项填空题