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.

1.solid

2.carbon dioxide

3.helium

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.