Styrene is produced by catalytic dehydrogenation of ethyl- benzene at high temperature in the presence of superheated steam.
Given the following data,
Ethylbenzene, C6H5--CH2CH3 :
delta Ht = -12.5 kJ/mol,
delta Gt = 119.7 kJ/mol and
S = 255 J/mol*K
Styrene, C6H5--CH==CH2 :
delta Ht = 103.8 kJ/mol,
delta Gt = 202.5 kJ/mol
and S = 238 J/mol*K
(a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: answer 116.3 kj, 82.8 kj, 114 j/k
(b) At what temperature is the reaction spontaneous? answer 747C
C)What are Delta G (answer 16.8 kj/m )
and K at 600 degrees?
Note: I only need help with K at 600 degrees. Thank you.
I know part of the answer is ^-2
What's your problem with using dG = -RT*ln K as I suggested earlier.
Look at your earlier post below. I think you just dropped the negative sign and didn't use enough significant figures.
To find K at 600 degrees, we can use the equation:
ΔG° = -RTlnK
Where ΔG° is the standard Gibbs free energy change, R is the gas constant (8.314 J/mol*K), T is the temperature in Kelvin, and K is the equilibrium constant.
Given that ΔG° is 16.8 kJ/mol and the temperature is 600 degrees, we first need to convert the temperature to Kelvin:
600 degrees Celsius = 873 Kelvin
Next, we convert ΔG° from kJ/mol to J/mol:
ΔG° = 16.8 kJ/mol = 16,800 J/mol
Now we can rearrange the equation to solve for K:
K = e^(-ΔG°/RT)
Plugging in the values:
K = e^(-16,800 J/mol / (8.314 J/mol*K * 873 K))
Calculating this expression will give you the value of K at 600 degrees.