For the equilibrium A(g)+2 B(g) ⇌C(g) the initial concentrations are [A]=[B]=[C]=0.100 atm . O

step 1 So continuing on with thermodynamics, we will firstly look at the equilibrium pressure for C. So

For the equilibrium A(g)+2 B(g) ⇌C(g) the initial...

For the equilibrium $$\mathrm{A}(g)+2 \mathrm{~B}(g) \rightleftharpoons \mathrm{C}(g)$$ the initial concentrations are $[\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=0.100 \mathrm{~atm} .$ Once equilibrium has been established, it is found that $[\mathrm{C}]=0.040 \mathrm{~atm}$. What is $\Delta G^{\circ}$ for this reaction at $25^{\circ} \mathrm{C}$ ?

For the equilibrium
$$\mathrm{A}(g)+2 \mathrm{~B}(g) \rightleftharpoons \mathrm{C}(g)$$
the initial concentrations are $[\mathrm{A}]=[\mathrm{B}]=[\mathrm{C}]=0.100 \mathrm{~atm} .$ Once equilibrium has been established, it is found that $[\mathrm{C}]=0.040 \mathrm{~atm}$. What is $\Delta G^{\circ}$ for this reaction at $25^{\circ} \mathrm{C}$ ?

Key Concepts

Standard Gibbs Free Energy Change (?G°)

The standard Gibbs free energy change, ?G°, is a thermodynamic quantity that indicates the spontaneity of a reaction under standard conditions. It is directly related to the equilibrium constant by the relation ?G° = -RT ln K, linking the thermodynamic and equilibrium properties of the reaction.

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible chemical reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of all reactants and products over time. This concept is fundamental in understanding how reactions balance out under given conditions and what definitions of equilibrium constants represent.

ICE Table Method

The ICE (Initial, Change, Equilibrium) table is a systematic tool used in chemistry to track the concentrations (or pressures) of reactants and products as a reaction proceeds to equilibrium. By organizing the initial values, the changes that occur, and the final equilibrium values, it simplifies the determination of unknown quantities and the calculation of equilibrium constants.

Equilibrium Constant (K)

The equilibrium constant, K, quantifies the ratio of the concentrations (or partial pressures) of products to reactants at equilibrium, each raised to the power of their stoichiometric coefficients. It is a central concept in chemical equilibrium that provides insight into the position of equilibrium and the extent to which a reaction proceeds under specified conditions.

Relationship Between ?G° and the Equilibrium Constant

This key concept establishes that the standard Gibbs free energy change and the equilibrium constant are interconnected through the equation ?G° = -RT ln K. This equation highlights that a large equilibrium constant corresponds to a negative ?G° (favorable reaction), while a small equilibrium constant corresponds to a positive ?G° (non-spontaneous reaction) under standard conditions.

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