# How much heat is liberated by the combustion of 206 g of hydrogen? DeltaH_(comb) = -286 kJ/mol

$n \left(\text{H}\right) = \frac{m}{M} = \frac{206 g}{1.00 g m o {l}^{-} 1} = 206 m o l$
"Energy Released" = DeltaH_(comb) xx n = -286kJmol^-1xx206mol=58916kJ=58900kJ("3s.f.")