The value of Δ r G ° for the reaction, CH 2 = CH 2 ( g ) + H 2 ( g ) ⇄ CH 3 − CH 3 ( g ) , has to be calculated. Whether the reaction is product favored or not under standard conditions has to be stated. Concept Introduction: The Gibbs free energy of a system is defined as the enthalpy of the system minus the product of the temperature times the entropy of the system. The Gibbs free energy of the system is a state function as it is defined in terms of thermodynamic properties that are state functions.

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Chapter 16, Problem 69QRT

(a)

Interpretation Introduction

Interpretation:

The value of ΔrG° for the reaction, CH2=CH2(g)+H2(g)⇄CH3−CH3(g), has to be calculated. Whether the reaction is product favored or not under standard conditions has to be stated.

Concept Introduction:

The Gibbs free energy of a system is defined as the enthalpy of the system minus the product of the temperature times the entropy of the system. The Gibbs free energy of the system is a state function as it is defined in terms of thermodynamic properties that are state functions.

(b)

Interpretation Introduction

Interpretation:

The equilibrium constant (KP) has to be calculated for the reaction, CH2=CH2(g)+H2(g)⇄CH3−CH3(g). A comment on the connection between sign of ΔrG° and value of KP.

Concept Introduction:

The Gibbs free energy of a system is directly related to the equilibrium constant of a reaction. The Gibbs free energy of the system is a state function as it is defined in terms of thermodynamic properties that are state functions. The symbol for equilibrium constant is KP.

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