[ganz]

The question is:

Zinc dissolves in acid according to the balanced reaction:

Zn(s) + 2H+(aq) ---> Zn2+(aq) + H2(g)

A sample of zinc is placed in the ice calorimeter described in the "Experiemental" section below.  If 0.0657g of zinc causes a decrease of 0.109 mL 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.


Any help with this problem would be greatly appreciated.

Thank you

[Dan]

I think the reduction in volume is due to the ice melting. You need to know the density of ice, the density of water (1 g/mL) and the enthalpy of fusion of ice.
 
Using the densities, you can work out how many moles of water melt, and then work out the enthalpy of this process from the enthalpy of fusion of ice.

You know how many moles of Zn you put in so this enthalpy value you worked out can then be scaled to 1 mol.