[trinhn812]

I think i did this wrong help? : thermodynamics delta H,S,G?
Consider the reaction: H2(g) + Br2(g) -->2HBr(g)
where DeltaH (standard state)= –103.8 kJ/mol. When 1.0 atm of H2(g) and 1.0 atm of Br2(g) are mixed in a 1.0L flask at 25°C and allowed to reach equilibrium, the molecules of H2 were counted using a very sensitive technique. 1.10 x 1013 molecules were found.
For this reaction calculate the values of K, Delta G, and Delta S.


So I did the T= H/S
298 = -103.8/S
S=.348
G= 0 because reaction goes to equilibrium
G=-RTlnK
1=K
??

[Yggdrasil]

So I did the T= H/S

This is not correct.  I assume you are rearranging the equation for the definition of the change in entropy:

dS = dq_rev/T

While ΔH = q for a reaction at constant pressure, the reaction that you are observing is not reversible along an isothermal path and you cannot simplify the equation to have a simple 1/T dependence on temperature.


Instead, I suggest starting with an ICE table to determine K.