. At 1500 K , the process is not spontaneous. However, the process I2( g) ⟶2 I(g) 0.10 atm

step 1 Hi guys, so problem 28 asks us to explain why at 1500k we have the reaction of iodine molecule t

. At 1500 K , the process is not spontaneous. However, the...

. At 1500 K , the process
is not spontaneous. However, the process
$$
\begin{gathered}
\mathrm{I}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{I}(\mathrm{g}) \\
0.10 \mathrm{~atm} \quad 0.10 \mathrm{~atm}
\end{gathered}
$$
is spontaneous at 1500 K . Explain.

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Key Concepts

Temperature Effect on Spontaneity

Temperature plays a crucial role in determining the spontaneity of a reaction. In processes where the entropy increases, high temperatures enhance the T?S term. This can overcome unfavorable enthalpy changes (positive ?H) and drive the overall free energy change (?G) to be negative, thus making the reaction spontaneous.

Gibbs Free Energy

Gibbs free energy is a thermodynamic potential that predicts whether a process is spontaneous under constant temperature and pressure. The equation ?G = ?H - T?S shows that even if the enthalpy change (?H) is positive (non-spontaneous tendency), a sufficiently large positive entropy change (?S) multiplied by temperature (T) can result in a negative ?G, indicating that the process is spontaneous.

Entropy

Entropy represents the measure of disorder or randomness in a system. In chemical processes, an increase in the number of gas particles or a dispersal of energy often results in a positive entropy change. This increase in entropy can drive processes to occur spontaneously, especially at elevated temperatures.

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