Question

Calculate the enthalpy change for the hydrolysis of sucrose given the following information: Sucrose (C12H22O11) reacts with water to form glucose (C6H12O6) and fructose (C6H12O6). Delta H for the reaction is -190 kJ/mol. The enthalpy of formation for sucrose is -2227 kJ/mol, the enthalpy of formation for glucose is -1274 kJ/mol, and the enthalpy of formation for fructose is -1266 kJ/mol.

Answer 1

To calculate the enthalpy change for the hydrolysis of sucrose, we can use the following equation:H_reaction =  H_f products  -  H_f reactants where H_reaction is the enthalpy change for the reaction, H_f products  is the sum of the enthalpies of formation of the products, and H_f reactants  is the sum of the enthalpies of formation of the reactants.For this reaction, the reactants are sucrose and water, and the products are glucose and fructose. The enthalpy of formation for water is not given, but since it is a reactant and not a product, it will not affect the final result.H_reaction = [H_f glucose  + H_f fructose ] - [H_f sucrose  + H_f water ]H_reaction = [ -1274 kJ/mol  +  -1266 kJ/mol ] - [ -2227 kJ/mol  + 0]H_reaction =  -2540 kJ/mol  -  -2227 kJ/mol H_reaction = 313 kJ/molThe enthalpy change for the hydrolysis of sucrose is 313 kJ/mol.