Consider the equilibrium

At 1000 K and a const. total pressure of 2 bar, C2H6 is introduced into a reaction vessel. the total pressure is held const. at 2 bar and at equilibrium the composition of the mixture in mole percent is H2(g): 20.4%, C2H4 (g): 20.4%, and C2H6 (g): 59.2%.

Calculate Kp at 1000 K

if ΔH of reaction = 137 kJ/mol, calculate the value of Kp at 298.15K

Calculate ΔG of reaction for this reaction at 298.15 K

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

Thus, Kp for this reaction is computed based on the given molar fractions and the total pressure at equilibrium, as shown below:

Now, by using the Van't Hoff equation one computes the equilibrium constant at 298.15K assuming the enthalpy of reaction remains constant:

Finally, the Gibbs free energy for the reaction at 298.15K is:

Best regards.

the answer is 1 i believe

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