Asked by Casey
So I have the reaction
2HBr(g) <--> H2(g)+Br2(g)
I'm supposed to find the equilibrium constant, K, using free energy (G) values. The values in my textbook for G of H2 and Br2 were zero, and the value for HBr(g) was -53.5.
So, to find delta G I did products - reactants and got (0+0)-(2(-53.5)) and got that the delta G is +107.
Next I plugged that into the equation
deltaG = -RTlnK.
107kJ/mol(1000J/1kJ) = -8.314(298K)lnK
-43.2 = lnK
K=1.75x10^-19
I thought that should be the answer, but my homework says it's wrong. What am I doing wrong here? I've done several others of the same type of problem and gotten them right, so I don't know what the difference is.
2HBr(g) <--> H2(g)+Br2(g)
I'm supposed to find the equilibrium constant, K, using free energy (G) values. The values in my textbook for G of H2 and Br2 were zero, and the value for HBr(g) was -53.5.
So, to find delta G I did products - reactants and got (0+0)-(2(-53.5)) and got that the delta G is +107.
Next I plugged that into the equation
deltaG = -RTlnK.
107kJ/mol(1000J/1kJ) = -8.314(298K)lnK
-43.2 = lnK
K=1.75x10^-19
I thought that should be the answer, but my homework says it's wrong. What am I doing wrong here? I've done several others of the same type of problem and gotten them right, so I don't know what the difference is.
Answers
Answered by
Casey
Nevermind . . . the G value for Br2 isn't 0, which was throwing off my calculations. The answer ended up being 4.96x10^-20
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