Consider the equilibrium c2h6(g) ↔ c2h4(g) + h2(g) . at 1000k and a constant total pressure of 1 bar, h2(g) is introduced into the reaction vessel. the total pressure is held constant at 1 bar and at equilibrium the composition of the mixture in mole percent is h2 : 26% ; c2h4: 26% ; c2h6 : 48%calclate kp at 1000 k.

Explanation:

From the reaction:

C₂H₆(g) ⇆ C₂H₄(g) + H₂(g)  

 48%          26%       26%

Knowing the composition of the mixture at equilibrium (at 1000K), we can calculate the equilibrium constant in terms of mole fraction:          

where X: mole fraction of C₂H₆(g), C₂H₄(g) and H₂(g)  

Now, the equilibrium constant in terms of pressure can be calculated using the equilibrium constant in terms of mole fraction:      

where : total pressure and Δn: number of gaseous moles of product - number of gaseous moles of reactant  

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answer; 4 electrons;