A possible reaction for converting methanol to ethanol is
CO(g)+2H2(g)+CH3OH(g)→C2H5OH(g)+H2O(g)
ΔH0 for this reaction at 25∘C.
ΔH0 = -165.7 kJ
ΔS0 for this reaction at 25∘C.
ΔS0 = -227.4 J/K
ΔG0 for this reaction at 25∘C.
ΔG0 = -97.9 kJ
- Estimate Kp for the reaction at 740 K .
Express your answer using two significant figures.
what i did
(-97.9kJ)(1000) = -(8.314)(740K) lnK
-97900 / -(8.314)(740K) = ln K
e^(-97900 / -(8.314)(740K)) = K
Kp = 8.1x10^6
The above answer is not correct. Plz help. Thanks
If you plug in 298 for T you will get Kp at 298. Then the van't Hoff equation will convert that to K at 740K.
ln(kt2/kt1) = dHo(1/T1-1/T2)/R
To estimate Kp for the reaction at 740 K, we can use the equation:
ΔG0 = -RT ln K
Where ΔG0 is the standard Gibbs free energy change, R is the ideal gas constant (8.314 J/(mol·K)), T is the temperature in Kelvin, and K is the equilibrium constant.
To solve for K, we rearrange the equation:
K = e^(-ΔG0 / (RT))
Now let's plug in the values we have:
ΔG0 = -97.9 kJ = -97900 J
R = 8.314 J/(mol·K)
T = 740 K
Substituting these values into the equation, we get:
K = e^(-(-97900) / (8.314 × 740))
Simplifying further:
K = e^(117.77)
Using a calculator or mathematical software, we find that e^(117.77) is a very large number, approximately 1.34 × 10^51.
Therefore, the estimated value of Kp for the reaction at 740 K is approximately 1.34 × 10^51.