Calculate the standard free energy change for the reaction, N2( g)+3 H2( g) ⟶2 NH3( g) at 298

step 1 we know that delta g not is equal to delta h0 minus t delta s not so delta g not is the standard

Calculate the standard free energy change for the reaction,...

Calculate the standard free energy change for the reaction, $$ \mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{~g})} \text { at } 298 \mathrm{~K} $$ Given $\Delta H^{\circ}=-92.4 \mathrm{~kJ}$ and $\Delta S^{\circ}=-198.3 \mathrm{JK}^{-1} .$ Also, comment on the result.

Calculate the standard free energy change for the reaction,
$$
\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{~g})} \text { at } 298 \mathrm{~K}
$$
Given $\Delta H^{\circ}=-92.4 \mathrm{~kJ}$ and $\Delta S^{\circ}=-198.3 \mathrm{JK}^{-1} .$ Also, comment on the
result.

Key Concepts

Gibbs Free Energy

Gibbs Free Energy is a thermodynamic potential that measures the maximum amount of useful work obtainable from a thermodynamic process at constant temperature and pressure. It is calculated using the equation ?G = ?H - T?S, which links the system’s enthalpy change (?H), entropy change (?S), and the absolute temperature (T). A negative ?G indicates that a process is spontaneous under given conditions.

Enthalpy Change (?H)

Enthalpy Change represents the heat absorbed or released during a reaction at constant pressure. It indicates whether a reaction is exothermic (releases heat, negative ?H) or endothermic (absorbs heat, positive ?H), affecting the energy balance of the process.

Entropy Change (?S)

Entropy Change refers to the change in disorder or randomness in a system as a result of a process. A decrease in entropy (negative ?S) suggests that the system is becoming more ordered, while an increase (positive ?S) indicates a rise in disorder. In the context of Gibbs Free Energy, the T?S term helps determine the temperature dependence of spontaneity.

Standard State Conditions

Standard State Conditions provide a reference framework for thermodynamic measurements, implying that substances are measured at a pressure of 1 bar for gases, concentrations of 1 mol/L for solutions, and the pure substance in its most stable form for solids and liquids. These conditions allow for consistent and comparable thermodynamic data across different reactions.

Thermodynamic Spontaneity

Thermodynamic Spontaneity is determined by the sign and magnitude of the Gibbs free energy change (?G). A reaction with a negative ?G is considered spontaneous under the defined conditions, meaning it can proceed without external energy input. The balance between enthalpy and entropy changes ultimately dictates the spontaneity of a reaction.

Transcript

Please give Ace some feedback