Posted by Rose Bud on .
calculate enthalpy of H for the reaction
N2H4(l) + 2H2O(l) > N2(g) + 4H2)(l)
Given the reactions
N2H4(l) + O2(g) > N2(g) + 2H2O(l) Enthalpy of H = 6.22.2 kJ
H2(g) + (1/2)O2(g) > H2O(l) enthalpy of H = 285.8 kJ/mol
H2(g) + O2(g) > H2O2(l) enthalpy of H = 187.8 kJ

chemistryThermochemistry (grade 12) 
DrBob222,
You need to check the post carefully. The equation you want is not balanced. I think you have made two typos. I think the left H2O should be H2O2 and I think the right H2) should be H2O

chemistryThermochemistry (grade 12) 
Rose Bud,
You are defiantly right.
it is suppose to be 2H2O2(l) and 4H2O(l)
and the first equation is suppose to be 622.2 kJ/mol
actually they are all suppose to be kJ/mol, but that was a typo on the exercise.
For a final answer I got 818.2 kJ/mol
i used the first equation as is. then i used the second equation and multiplied it by two and then for the last equation i reversed it and also multiplied it by 2. 
chemistryThermochemistry (grade 12) 
Anonymous,
N2 + 2F2 > 2NF3 calculate the standard enthalpy