Question

Calculate the enthalpy change for the hydrolysis of 2 moles of sucrose (C12H22O11) given the standard enthalpies of formation of sucrose, glucose, and fructose are -2220 kJ/mol, -1274 kJ/mol, and -915 kJ/mol respectively.

Answer 1

To calculate the enthalpy change for the hydrolysis of 2 moles of sucrose, we can use the following equation:H = H products  - H reactants The hydrolysis of sucrose can be represented by the following balanced chemical equation:C12H22O11 + H2O  C6H12O6  glucose  + C6H12O6  fructose Now, we can plug in the given standard enthalpies of formation:H = [ -1274 kJ/mol  +  -915 kJ/mol ] - [ -2220 kJ/mol ]H =  -2189 kJ/mol  -  -2220 kJ/mol H = 31 kJ/molSince we are calculating the enthalpy change for the hydrolysis of 2 moles of sucrose, we need to multiply the enthalpy change per mole by 2:H_total = 31 kJ/mol  2 molesH_total = 62 kJTherefore, the enthalpy change for the hydrolysis of 2 moles of sucrose is 62 kJ.