Maximum temperature attainable by thermite reaction In the thermite reaction
  $$\ce{2Al(s) + Fe2O3(s) -&gt; 2Fe(l) + Al2O3(s)}$$
  what is the maximum temperature attainable by the products? Assume reactants at $25\ \mathrm{^\circ C}$ and $1\ \mathrm{atm}$ and that all heat capacities remain constant.


I started by using Hess's law to find the enthalpy change of the reaction. I couldn't find a heat of formation for liquid iron so I assume I have to find that out. I just wrote out the equation
$$\ce{Fe(s) + heat + enthalpy of fusion -&gt; Fe(s)}$$
and figured the heat of formation for liquid iron at $25\ \mathrm{^\circ C}$ is around $-302.71\ \mathrm{kJ/mol}$. 

To find the max temperature I used 
$$\Delta H_\mathrm r=\Delta T\cdot C_\mathrm p(\text{products})$$
and came out with an equation like 
$$-14445\ \mathrm{kJ/mol}=0.147\ \mathrm{kJ/(mol\ K)}\cdot T_\text{max}$$
This gives me a negative temperature, so I assume it is wrong. Even if I were to take the absolute value, the answer seems awfully high. I was expecting something around a few thousand degrees not near ten thousand.
According to Wikipedia the maximum temperature is approximately 2500 °C, limited by the boiling point of aluminum, which is 2519 °C.  The article provides some discussion of how the temperature is limited, and how to calculate it using Hesse's law.