Question
Asked Sep 7, 2019
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Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is

C2H2(g)+2H2(g)⇌C2H6(g)

Given the following data at standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K), what is the value of Kp for this reaction?

Substance G∘f
(kJ/mol)
C2H2(g) 209.2
H2(g) 0
C2H6(g) −32.89
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Expert Answer

Step 1

The given reaction is:

C2H2 (g) + 2H2 (g) ═ C2H6 (g)

 

The standard free energy change of the given reaction is calculated by subtracting the standard free energies of formation of reactants from that of the products.

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G =G; (C,H,(8))-G;(C,H(8) + 2G; (H (8)] cg 6 =(-32.89 kJ/mol)-(209.2 kJ/mol +2x0 kJ/mol) =-242.09 kJ/mol

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Step 2

The conversion factor for kJ/mol and J/mol units is:

1 kJ/mol = 103 J/mol

 

Hence, -242.09 kJ/mol = -242.09 × 103 J/mol

                                                   = -242090 J/mol

Step 3

The relation between equilibrium constant and standard free energy change is given in the equation (1) in which ΔG0 is the standard free energy change, R is the universal gas const...

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AG RT n K .. (1) 242090 J/mol -(8.314 J/molK )(298 K ) In K -242090 J/mol InK -(8.314 J/molK) (298 K) (2) n K 97.71 K 2.73x 1042

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