Acetylene, C_2H_2, can be converted to ethane, C_2H_6, by a process known as hyd

Question

Acetylene, C_2H_2, can be converted to ethane, C_2H_6, by a process known as hydrogenation. The reaction is C_2H_2 (g) + 2H_2(g) C_2H_6 (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 K_p for this reaction? Express your answer using two significant figures. In Part A, we saw that Delta G degree = -242.1 kJ for the hydrogenation of acetylene under standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K). In Part B, you will determine the Delta G for the reaction under a given set of nonstandard conditions. At 25 degree C the reaction from Part A has a composition as shown in the table below. What is the free energy change, Delta G, in kilojoules for the reaction under these conditions? Express your answer numerically in kilojoules.

Explanation / Answer

part B

dG = dG0 +RTln(pC2H6/pH2*pC2H2)

dg0 = -242.1 Kj

pC2H6 = 0.0425 atm

pH2 = 4.45 atm

pC2H2 = 3.95 atm

DG = (-242.1*10^3)+(8.314*298)ln(0.0425/(4.45*3.95))

   = -257 kj

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