1a) For a reaction, a plot of ln K versus inverse temperature is found to be linear and fits the following equation: y = -1,714x + 5.64. What is the value of ΔH? Give your answer with units of kJ/molK; however, you should not type in the units
b) If you find that the standard Gibbs free energy change for a reaction is 1.98 kJ/molK, what is the equilibrium constant for the reaction at 25.0 oC? Be careful with your units in the calculation.
1)
The relation between K and T is:
K = A*e^(-Ho/RT)
taking ln on both sides, above expression becomes,
ln K = ln A - Ho/RT
So, slope between ln K and 1/T will have a value of -Ho/R and y intercept is ln A
So, Ho can be calculated from slope
slope = -Ho/R
-1714 = -Ho/8.314
Ho = 1.43*10^4 J/mol
Ho = 14.3 KJ/mol
Answer: 14.3
2)
T= 25.0 oC
= (25.0+273) K
= 298 K
ΔGo = 1.98 KJ/mol
ΔGo = 1980 J/mol
use:
ΔGo = -R*T*ln Kc
1980 = - 8.314*298.0* ln(Kc)
ln Kc = -0.7992
Kc = 0.4497
Answer: 0.450
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