|Feb15-09, 12:59 PM||#1|
heat enthalpy of molecular hydrogen
1. The problem statement, all variables and given/known data
Look up the enthalpy of formation of atomic hydrogen in the back of the book. This is the enthalpy change when a mole of atomic hydrogen is formed by dissociating 1/2 mole of molecular hydrogen (the more stable state of the element). From this number, determinethe energy needed to dissociate a single H2 molecule , in electron-volts.
2. Relevant equations
3. The attempt at a solution
found delta(H) to be delta(H)=-217.97 kJ
According to the standard table T=298 K and P=1 bar=1atm?
PV=RT=(8.31 J/K)(298 K)=2.5 kJ
H-PV=(-217.97 kJ)-(2.5 kJ)=-220.5 kJ
Did I find delta(U) correctly?
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