Answer:
Explanation:
<u>From the reaction:</u>
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:
<em>where </em><em>X: mole fraction of C₂H₆(g), C₂H₄(g) and H₂(g) </em>
Now, the equilibrium constant in terms of pressure can be calculated using the equilibrium constant in terms of mole fraction:
<em>where </em><em>: total pressure</em><em> and </em><em>Δn: number of gaseous moles of product - number of gaseous moles of reactant </em>
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