(adsbygoogle = window.adsbygoogle || []).push({}); 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?

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# Heat enthalpy of molecular hydrogen

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