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 PV=3100 J delta(H)=delta(U)+P*delta(V) H=U+PV 3. The attempt at a solution find delta(U) delta(U)=delta(H)-P*delta(V) found delta(H) to be delta(H)=-217.97 kJ According to the standard table T=298 K and P=1 bar=1atm? R=8.31 J/K 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?