Explanation The equilibrium constant of the reactions can be determined as- Reaction 1: The wrong calculations made by the group of students. Δ G 0 = − R T ln K 1 . On plugging the values: ( − ) 50 = ( − ) 8.314 J o u l e / K × ( 25 + 273 ) K × 2.303 × log K 1 K 1 = 1.018 The correct process: Δ G 0 = − R T ln K 1 On plugging the given values, ( − ) 50 × 10 3 J o u l e = ( − ) 8.314 J o u l e / K × ( 25 + 273 ) K × 2.303 × log K 1 log K 1 = 50 × 10 3 8.314 × 298 × 2.303 K 1 = 5.78 × 10 8 Reaction 2: Δ G 0 = − R T ln K 2 The wrong calculations made by the group of students. Δ G 0 = − R T ln K 2 . On plugging the values: ( − ) 30 = ( − ) 8.314 J o u l e / K × ( 25 + 273 ) K × 2.303 × log K 2 K 2 = 1.011 The correct process: Δ G 0 = − R T ln K 2 On plugging the given values, ( − ) 30 × 10 3 J o u l e = ( − ) 8

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ISBN: 9781337398909

Author: Lawrence S. Brown, Tom Holme

Publisher: Cengage Learning

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Chapter 12, Problem 12.79PAE

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The error made by the group of the students to determine the equilibrium constant of the reactions and the actual values of equilibrium constants of the reactions.

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Chapter 12, Problem 12.78PAE

Chapter 12, Problem 12.80PAE

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The error made by the group of the students to determine the equilibrium constant of the reactions and the actual values of equilibrium constants of the reactions.

Solution Summary: The author explains that the unit calculation is as important as the numerical values of equilibrium constants of reactions.

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To determine: The error made by the group of the students to determine the equilibrium constant of the reactions and the actual values of equilibrium constants of the reactions.

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Chapter 12 Solutions

To determine:

The error made by the group of the students to determine the equilibrium constant of the reactions and the actual values of equilibrium constants of the reactions.