At room temperature (25^∘ C), the gas CINO is impure because it decomposes slightly according to

step 1 To determine the delta G standard for this reaction at 25 degrees Celsius or 298 Kelvin, we need

At room temperature (25^∘ C), the gas CINO is impure because...

At room temperature $\left(25^{\circ} \mathrm{C}\right)$, the gas CINO is impure because it decomposes slightly according to the equation $$ 2 \mathrm{CINO}(g) \rightleftharpoons \mathrm{Cl}_{2}(g)+2 \mathrm{NO}(g) $$ The extent of decomposition is about $5 \%$. What is the approximate value of $\Delta G_{298}^{\circ}$ for this reaction at this temperature?

At room temperature $\left(25^{\circ} \mathrm{C}\right)$, the gas CINO is impure because it decomposes slightly according to the equation
$$
2 \mathrm{CINO}(g) \rightleftharpoons \mathrm{Cl}_{2}(g)+2 \mathrm{NO}(g)
$$
The extent of decomposition is about $5 \%$. What is the approximate value of $\Delta G_{298}^{\circ}$ for this reaction at this temperature?

Key Concepts

Standard Gibbs Free Energy Change (?G°)

This represents the change in Gibbs free energy when a reaction occurs under standard conditions (usually 1 bar pressure for gases, 1 M for solutions, and pure substances for solids/liquids). It provides a measure of the inherent driving force or spontaneity of a chemical reaction, independent of the concentrations or pressures of reactants and products at the time of measurement.

Equilibrium Constant (K)

The equilibrium constant quantifies the ratio of the concentrations or partial pressures of products to reactants at equilibrium for a given reaction, taking into account the stoichiometry of the reaction. It is a fundamental parameter in chemical thermodynamics that helps determine the position of equilibrium.

Relationship Between ?G° and Equilibrium Constant

There is a direct connection between the standard Gibbs free energy change and the equilibrium constant, expressed by the equation ?G° = -RT ln K. This relationship allows one to calculate the thermodynamic favorability of a reaction based on its equilibrium position, and vice versa.

Reaction Stoichiometry and Extent of Reaction

Stoichiometry relates the quantities of reactants and products in a chemical reaction. In cases where only a small fraction of reactants converts to products (i.e., a limited extent of decomposition), stoichiometric considerations are crucial for determining the equilibrium concentrations or pressures, which in turn are used to calculate the equilibrium constant.

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