[Mayhem101]

Zinc dissolves in acid according to the balanced chemical reaction:

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

A sample of zinc is placed in the ice calorimeter described in the "Experimental" section (I'll specify 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.

The calorimeter details:

T = constant

density of water = 1.000 g mL-1

density of ice = 0.917 g mL-1

It states further on that, "Given that the enthalphy change for the process H2O (s) --> H20 (l) is 6.01 kJ/mol or 333 J/g, it can be determined that 3.68 kJ are released per mL change in the volume of the ice/water mixture."

H2O (s) -> H2O (l) deltaH of fusion = 6.01 kJ mol-1, or 333 J g-1
--------------------------------------------------------------

So, isn't this all I need to do?

Amount of moles for Zn = 0.0657g / 65.39 g mol-1 = 0.001 mol
0.109mL x 3.68 kJ mL-1 = 0.401 kJ
0.401 kJ / 0.001 mol = 401 kJ mol-1

[Borek]

Correct approach, but you should watch your significant digits. 0.001 mol suggests much lower accuracy than that given by 0.0657 g.