Free energy and equilibrium

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The gas-phase isomerization of cis-

2

-butene to produce trans-

2

-butene is represented by the equation above. The value of the standard free energy change,

Δ G °_{r x n}

, for the reaction is

- 3.05 {kJ/mol}_{r x n}

298 K

Calculate the value of the equilibrium constant, $K_{e q}$ ‍, for the reaction at $298 K$ ‍.
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The AP Chemistry exam includes a section of equations and constants that you can reference during the exam. A subset of this reference is shown below.

Gibbs free energy equations:

\begin{aligned} Δ G °_{r x n} & = Δ H °_{r x n} - T Δ S °_{r x n} \\ = - R T \ln K \end{aligned}

Gibbs free energy variables and constants:

\begin{aligned} G ° & = standard Gibbs free energy \\ H ° & = standard enthalpy \\ S ° & = standard entropy \\ T & = temperature \\ K & = equilibrium constant \end{aligned}

\begin{aligned} Gas constant, R & = 8.314 J {mol}^{- 1} K^{- 1} \end{aligned}

AP®︎/College Chemistry

Course: AP®︎/College Chemistry > Unit 9

Problem