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RJLiberator
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Homework Statement
Dinitrogen tetroxide decomposes to nitrogen dioxide:
N2O4(g)→2NO2(g) ΔHorxn=55.3kJ
At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2.
What percentage of N2O4 decomposes at 370K ? Assume that the initial pressure of N2O4 is the same (0.100 atm).
How is this problem done?
We know:
Delta H of reaction = 55.3 kJ
Equilibrium means Delta G = 0 AT 298 K and 58% decomposition.
We need to find what percentage of N2O4 decomposes at 370K.
I'm not entirely sure what equations I should be using. We are talking about Gibbs Free Energy. This is a mast. chem. problem and the last of the 40-50 I have left.
If someone could guide me towards a correct equation, I can work this out.