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Consider the following reaction:

2H2 (g) + O2 (g)  2H2O (l) ΔH = -572 kJ
a. How much heat is evolved for the production of 1.00 mol H2O (l)?
b. How much heat is evolved when 4.03 g hydrogen is reacted with excess oxygen?
c. How much heat is evolved when 186 g oxygen is reacted with excess hydrogen?
d. The total volume of hydrogen gas needed to fill the Hindenburg was 2.0 x 10
8
L at 1.0 atm
and 25
o
C. How much heat was evolved when the Hindenburg exploded, assuming all of the
hydrogen reacted?

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1 answer
  1. a. 572 kJ/2
    b. 572 kJ/mol x (4.03/4) = ?

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