Question

In: Chemistry

PART A. Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation....

PART A.

Acetylene, C2H2, can be converted to ethane, C2H6, by a process known as hydrogenation. The reaction is

C2H2(g)+2H2(g)⇌C2H6(g)

All pressures equal to 1 atm and the common reference temperature 298 K, What is Kp?

Substance ΔG∘f
(kJ/mol)
C2H2(g) 209.2
H2(g) 0
C2H6(g)

−32.89

PART B.

At 25 ∘C the reaction from Part A has a composition as shown in the table below.

Substance Pressure
(atm)
C2H2(g) 4.95
H2(g) 5.65
C2H6(g) 1.25×10−2

What is the free energy change, ΔG, in kilojoules for the reaction under these conditions?

Solutions

Expert Solution

Here asked free energy change

∆G = ∆G° + RTlnK

∆G° = -242.09 kJ / mol ( from part A)

∆G = -242.09 kJ / mol -23.4 kJ/mol

∆G = -265.49 kJ


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