At equilibrium, the change in Gibbs free energy (ΔG) is zero, indicating that the system is at maximum entropy.

For a reversible process, the change in entropy (ΔS) is given by ΔS = Q/T, where Q is the heat absorbed and T is the temperature.

The change in entropy (ΔS) for a reversible process is given by ΔS = Q/T, where Q is the heat absorbed and T is the temperature.

For a reversible process, the change in entropy of the universe is zero, as the system and surroundings are in equilibrium.

For a spontaneous process, the total entropy change of the universe (system + surroundings) must be positive.

The correct relationship is ΔG = ΔH - TΔS, where ΔG must be negative for a spontaneous process.

The relationship is given by ΔG = ΔH - TΔS, where ΔG must be negative for a spontaneous process.

For a process to be spontaneous, the change in Gibbs free energy (ΔG) must be negative.

The change in entropy ΔS = Q/T = 100 J / 300 K = 0.33 J/K.

An increase in entropy indicates that the process is spontaneous, as per the second law of thermodynamics.

As the temperature of a system increases, the kinetic energy of the particles increases, leading to greater disorder and thus an increase in entropy.

In a closed system, an increase in temperature generally leads to an increase in entropy, as the molecular motion becomes more chaotic.

In an irreversible process, the change in entropy of the universe is positive, indicating that the total entropy increases.

The reaction N2(g) + 3H2(g) → 2NH3(g) results in a decrease in the number of gas molecules, leading to a negative change in entropy.

The entropy of the system decreases when water freezes, as the molecules become more ordered in the solid state.

When a gas is compressed, the number of microstates decreases, leading to a decrease in entropy.

For a phase transition at constant temperature, the change in entropy is given by ΔS = ΔH/T, where ΔH is the enthalpy change.

The change in entropy for a reaction is calculated using the formula ΔS = ΣS(products) - ΣS(reactants).

According to the third law of thermodynamics, the entropy of a perfect crystal at absolute zero is zero.

According to the third law of thermodynamics, the entropy of a perfect crystal at absolute zero is zero, which is the minimum value.

The third law of thermodynamics states that the entropy of a perfect crystal approaches zero as the temperature approaches absolute zero.

According to the third law of thermodynamics, the entropy of a perfect crystal at absolute zero is exactly zero.

The third law of thermodynamics states that the entropy of a perfect crystalline substance approaches zero as the temperature approaches absolute zero.

According to the third law of thermodynamics, the entropy of a perfect crystalline substance at absolute zero is zero.

The change in entropy for an isothermal and reversible expansion of an ideal gas is given by ΔS = nR ln(V2/V1). For 1 mole, n = 1, hence ΔS = R ln(V2/V1).

The change in entropy for an isothermal expansion of an ideal gas is given by ΔS = nR ln(V2/V1). For 1 mole, it simplifies to ΔS = R ln(V2/V1).

Increasing temperature generally increases the kinetic energy of particles, leading to greater disorder and thus an increase in entropy.

As temperature increases, the kinetic energy of particles increases, leading to greater disorder and thus higher entropy.

During a phase transition at constant temperature, the change in entropy is given by ΔS = Q/T, where Q is the heat absorbed or released.

The entropy change for an isothermal expansion is given by ΔS = nR ln(V2/V1). For 1 mole, ΔS = R ln(V2/V1).