Which of the following statements is not truc? (1) All...

Which of the following statements is not truc? (1) All naturally occurring processes proceed spontaneously in the direction which leads to decrease in Gibbs energy. (2) For an endothermic reaction to be spontaneous, $\Delta(i>0$ (3) For the reversible vaporisation of water at $100^{\circ} \mathrm{C}$ and I atmospheric pressure, $\Delta G$ is equal to zero. (4) If $\Delta\left(j^{n}>0\right.$ for a reaction, then $k_{p}<1$.

Which of the following statements is not truc?
(1) All naturally occurring processes proceed spontaneously in the direction which leads to decrease in Gibbs energy.
(2) For an endothermic reaction to be spontaneous, $\Delta(i>0$
(3) For the reversible vaporisation of water at $100^{\circ} \mathrm{C}$ and I atmospheric pressure, $\Delta G$ is equal to zero.
(4) If $\Delta\left(j^{n}>0\right.$ for a reaction, then $k_{p}<1$.

Key Concepts

Relationship Between Gibbs Free Energy and Equilibrium Constant

The standard Gibbs free energy change is thermodynamically related to the equilibrium constant (K) through the equation ?G° = -RT ln K. This relationship shows that a negative ?G° corresponds to an equilibrium constant greater than one (favoring products), whereas a positive ?G° results in an equilibrium constant less than one (favoring reactants), providing a quantitative link between thermodynamics and reaction yields.

Temperature, Enthalpy, and Entropy Relationship

The spontaneity of a reaction is influenced not only by the enthalpy change but also by the entropy change of the system. Even endothermic reactions (with positive enthalpy change) can be spontaneous if the increase in entropy (?S) is sufficient, particularly at higher temperatures, such that the T?S term overcomes the enthalpy term, resulting in a negative ?G.

Chemical Equilibrium

Chemical equilibrium occurs when the forward and reverse reaction rates are equal, resulting in no net change in the concentration of reactants and products. At equilibrium, the system's Gibbs free energy is minimized and remains constant (?G = 0), indicative of a balanced, reversible process.

Gibbs Free Energy

Gibbs free energy is a thermodynamic potential defined as G = H - TS, combining enthalpy (H) and entropy (S) at a given temperature (T) to determine the feasibility of a process. A decrease in Gibbs free energy (negative ?G) at constant temperature and pressure indicates that a process or reaction can occur spontaneously, while ?G = 0 denotes equilibrium.

Spontaneous Process

A spontaneous process is one that occurs naturally without the input of external energy, driven by the tendency to lower the system's free energy. Spontaneity is characterized by a negative change in Gibbs free energy for reactions and processes, meaning that the overall system moves toward a more stable, lower-energy state.

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