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.