Styrene is produced by catalytic dehydrogenation of ethyl- benzene at high temperature in the presence of superheated steam. (a) Find ÄH°rxn, ÄG °rxn, and ÄS °rxn, given these data at 298 K: (b) At what temperature is the reaction spontaneous?
What are Delta G and K at 600 degrees?
I only need help with K at 600 degrees. Thank you. I thought it was 9.9 x 10^2 but it was marked wrong.
data:
Given the following data, what is the delta Hrxn, delta Grxn and delta Srxn at 298 K. 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
To find K at 600 degrees, we can use the equation:
ΔG = ΔH - TΔS
Where:
ΔG: Gibbs Free Energy
ΔH: Enthalpy
ΔS: Entropy
T: Temperature (in Kelvin)
Given that you want to find K at 600 degrees, which is 873 Kelvin (600 + 273), we can use the equation:
ΔG = -RT ln(K)
Where:
R: Gas constant (8.314 J/(mol·K))
ln: Natural logarithm
K: Equilibrium constant
Now, solving for K:
K = e^(-ΔG/RT)
Plugging in the given values:
T = 873 K
ΔG = -9.9 x 10^2 J/mol
R = 8.314 J/(mol·K)
K = e^(-(-9.9 x 10^2)/(8.314 * 873))
Calculating this expression, we get:
K ≈ 2.6 x 10^10
So the approximate value of K at 600 degrees is 2.6 x 10^10.