The determination of value of Δ G was done by using the concept of Gibbs free energy. Concept introduction: In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces. Given: Here, we have the formation of ethylene. The partial pressure of the reactant (H 2 = 100 atm) and product (C 2 H 4 = 0.10 atm) and value of Δ G o (= 68.1 KJ) are given. We need to find out the direction in which the reaction is spontaneous.

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Chapter 17, Problem 17.17P

Interpretation Introduction

Interpretation:

The determination of value of ΔG was done by using the concept of Gibbs free energy.

Concept introduction:

In a thermodynamics system, the Gibbs free energy is the thermodynamic potential used to determine the maximum quantity of non-expanding work that can be performed by a thermodynamically closed system (no exchange of energy and work with the surroundings), which can only be achieved during a reversible reaction. When a thermodynamic system reversibly transforms from one state to another, then the reduction in the amount of Gibbs free energy is equal to the amount of work done by the system to the surrounding, taking away the work of the pressure forces.

Given: Here, we have the formation of ethylene. The partial pressure of the reactant (H₂ = 100 atm) and product (C₂H₄ = 0.10 atm) and value of ΔGo (= 68.1 KJ) are given. We need to find out the direction in which the reaction is spontaneous.

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