Question

Calculate the enthalpy change for the hydrolysis of 2 moles of sucrose (C12H22O11) in aqueous solution given that the heat capacity of the solution is 4.18 J/g.K, the initial and final temperatures of the solution are 22.0°C and 28.0°C respectively. The molar mass of sucrose is 342.3 g/mol.

Answer 1

To calculate the enthalpy change for the hydrolysis of 2 moles of sucrose, we can use the formula:H = mcTwhere H is the enthalpy change, m is the mass of the solution, c is the heat capacity of the solution, and T is the change in temperature.First, let's find the mass of 2 moles of sucrose:mass = moles  molar massmass = 2 moles  342.3 g/molmass = 684.6 gNow, let's find the change in temperature:T = T_final - T_initialT = 28.0C - 22.0CT = 6.0CNow we can calculate the enthalpy change:H = mcTH =  684.6 g  4.18 J/g.K  6.0C H = 17116.968 JSince the enthalpy change is positive, the reaction is endothermic. The enthalpy change for the hydrolysis of 2 moles of sucrose in aqueous solution is 17,116.968 J or 17.12 kJ  rounded to two decimal places .