Question
The total volume of hydrogen gas needed to fill the Hidenbrug was 2.0e8 L at 1.0 atm and 25 degrees Celsius. How much heat was evolved when the Hidenburg exploded, assuming all the hydrogen reacted?
I will be happy to critique your thinking on this. First, calculate the moles of H2 used.
2.0e8 L H2/22.4 L H2 = 8.9e6 mol H2
For every 2 mol H2 used -572 kJ of energy is produced
-572 kJ/2 mol H2 = -2.86e2 kJ/mol
yes.
I have a balanced equation with this problem. It is:
2 H2 + O2 --> 2 H2O
(where the change in heat is -572 kJ)
I have to discover the heat that is evolved from this equation. Would you have to convert the moles of H2 to kJ of energy using stoichiometry?
I will be happy to critique your thinking on this. First, calculate the moles of H2 used.
2.0e8 L H2/22.4 L H2 = 8.9e6 mol H2
For every 2 mol H2 used -572 kJ of energy is produced
-572 kJ/2 mol H2 = -2.86e2 kJ/mol
yes.
I have a balanced equation with this problem. It is:
2 H2 + O2 --> 2 H2O
(where the change in heat is -572 kJ)
I have to discover the heat that is evolved from this equation. Would you have to convert the moles of H2 to kJ of energy using stoichiometry?