Zn(s) + 2H +(aq) -- Zn 2+(aq) + H2(g)

A sample of zinc is placed in the ice calorimeter described in the "experimental" section below. If 0.0657g of zinc causes a decrease of 0.109mL in the ice/water volume of the calorimeter, what is the enthalpy change , per mole of Zinc, for the above reaction per mole of zinc.

It is also given that enthalpy change for process H20(s) - H20(l) is +6.01kJ/mol or 333J/g and it can be determined that 3.68 kJ are released per mL change in volume of ice/water mixture.

I got 4.01 x 10^-4kJ/mol but just wanted to confirm if it was correct.

Question

Zn(s) + 2H +(aq) --> Zn 2+(aq) + H2(g)

A sample of zinc is placed in the ice calorimeter described in the "experimental" section below. If 0.0657g of zinc causes a decrease of 0.109mL in the ice/water volume of the calorimeter, what is the enthalpy change , per mole of Zinc, for the above reaction per mole of zinc.

It is also given that enthalpy change for process H20(s) -> H20(l) is +6.01kJ/mol or 333J/g and it can be determined that 3.68 kJ are released per mL change in volume of ice/water mixture.

I got 4.01 x 10^-4kJ/mol but just wanted to confirm if it was correct.