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Answer :
Final answer:
The question is about finding the value of the equilibrium constant at 500K employing the Van’t Hoff equation. The specific temperature, 500K, the equilibrium constant at 298K, and the enthalpy change values are plugged into the equation. However, Gibbs Free Energy, though given, isn't needed in this problem.
Explanation:
The problem given involves the calculation of the equilibrium constant, K, at a specific temperature of 500K. To find this, we can employ the Van’t Hoff equation which describes the temperature dependence of equilibrium constants. The equation is: ln(K₂/K₁) = -ΔH/R (1/T₁ - 1/T₂).
In this equation, K is the equilibrium constant, R is the ideal gas constant (8.314 J/K mol), T represents temperatures in Kelvin, and ΔH is the enthalpy change of the reaction.
Given that ΔH is 80.3 kJ/mol, we can convert this to J/mol by multiplying by 1000 to get 80300 J/mol. However, ΔG, the Gibbs Free Energy, isn't needed in this problem.
In this case, K₁ is given at 298K and equals 0.090.
We want to find K₂ at 500K. Rearranging the Vant Hoff equation to solve for K2, and plugging in the known values leads to K2 = K1 * exp[-ΔH/R * (1/T2 - 1/T1)]. Now just solve this equation to find the value of K2.
Learn more about Equilibrium Constants here:
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