Thermodynamics help! Ethylene reacts with steam to form ethanol at a constant pr

Question

Thermodynamics help!

Ethylene reacts with steam to form ethanol at a constant pressure of 1.5 bar and a constant temperature of 298 K in the following reaction: C2H4 + H2O = C2H5OH At 298 k, the standard Gibbs free energy of formation is -167.73 KJ/mol for ethanol, +68.48 KJ/mol for ethylene, and -228.42 KJ/mol for steam. The reactor initially contains zero moles of ethylene and steam, and one mole of ethanol. Derive a quadratic equation for the equilibrium reaction conversion (don't need to solve it). Assume ideal gases.

Explanation / Answer

C2H4 + H2O -------> C2H5OH

delta G0rkn = delta G0f C2H5OH - delta G0f C2H4 - delta G0f H2O = -7.79 kJ

Now, delta G0rkn = -R*T*lnKeq

-7790 = -8.314*298*lnKeq

or, lnKeq = 3.144

or, Keq = 23.196

Now, Keq = [C2H5OH]/{[C2H4]*[H2O]}

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