${\mathrm{SF}}_4\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\to {\mathrm{SO}}_2\left(\mathrm{g}\right)+4\mathrm{HF}\left(\mathrm{g}\right);\mathrm{\Delta H}=-828\mathrm{kcal}$

Which of the following statements accurately describes the above reaction?

This reaction is never thermodynamically favoured

The temperature of the surroundings will increase as this reaction 

$H_{2}O\left(l\right)$ will always be the limiting reagent

The entropy of the reactants exceeds that of the products