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

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Answer 1 · 2016-07-06T05:01:22

58900kJ

$n("H")=m/M=(206g)/(1.00gmol^-1)=206mol$

$"Energy Released" = DeltaH_(comb) xx n = -286kJmol^-1xx206mol=58916kJ=58900kJ("3s.f.")$

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