Assertion (A): For any chemical reaction at a particular temperature, the equilibrium constant is fixed and is

NCERT Exemplar · Q47

Q. Assertion (A): For any chemical reaction at a particular temperature, the equilibrium constant is fixed and is a characteristic property. Reason (R): Equilibrium constant is independent of temperature.

(i) Both A and R are true and R is correct explanation of A.

(ii) Both A and R are true but R is not correct explanation of A.

(iii) A is true but R is false.

(iv) Both A and R are false.

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Concept understanding — Phase Equilibrium

Phase Equilibrium: From Intuition to Precision

Imagine a glass of ice water on a warm day. The ice cubes are melting, but the water around them stays cold. If you wait long enough, the ice stops melting — not because the room got colder, but because the system has reached a balance. The ice and water coexist without any net change. That balance is phase equilibrium.

The Intuition: A Tug-of-War Between Two Tendencies

Every substance wants to exist in the phase (solid, liquid, or gas) that has the lowest energy under the given conditions. But there's a catch: nature also loves disorder (entropy). A solid is low-energy but highly ordered; a gas is high-energy but very disordered. At a specific temperature and pressure, these two opposing drives — minimising energy and maximising disorder — exactly cancel each other out. The result? Two phases can coexist peacefully, with molecules constantly jumping between them but no net change in the amount of each phase.

Think of it as a tug-of-war. On one side, molecules in the solid phase are tightly bound and low in energy. On the other side, molecules in the liquid phase have more freedom and higher entropy. At the melting point, the rope doesn't move — the rates of melting and freezing are equal.

The Precise Statement

Phase equilibrium is the condition in which two or more phases of a substance coexist in thermodynamic equilibrium, with no net transfer of mass between phases. For a pure substance, this occurs at a unique temperature for a given pressure (or vice versa), defined by the equality of the chemical potential (or Gibbs free energy per mole) in all phases.

In simpler terms: at equilibrium, the driving force for a molecule to move from phase A to phase B is exactly the same as the driving force to move from B to A. The system is dynamic — molecules are still crossing the boundary — but macroscopically static.

The Key Condition: Equal Chemical Potential

The rigorous condition for phase equilibrium in a pure substance is:

\mu_{\text{solid}} = \mu_{\text{liquid}} = \mu_{\text{gas}}

where $\mu$ (mu) is the chemical potential — the Gibbs free energy per mole. When chemical potentials are equal, no phase has a "preference" to grow at the expense of another.

Important

For a pure substance, phase equilibrium occurs only along specific lines on a phase diagram (the melting curve, boiling curve, and sublimation curve). At the triple point, all three phases coexist.

A Concrete Example: Water at 0°C

At 1 atm pressure and 0°C, ice and liquid water are in equilibrium. Here's what's happening at the molecular level:

Water molecules at the surface of the ice are vibrating. Some gain enough energy to break free and enter the liquid.
Simultaneously, water molecules in the liquid near the ice surface lose energy and attach to the ice crystal.
The rates of these two processes are equal. So the amount of ice and the amount of liquid water remain constant — even though individual molecules are constantly switching sides. …

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The equilibrium constant $K$ is indeed fixed at a given temperature and is a characteristic property of a reaction, but it changes with temperature. The assertion is true; the reason is false. The answer is (iii).

Why equilibrium constants matter

Every reversible reaction reaches a state where the forward and reverse rates balance. At this equilibrium, the ratio of product concentrations to reactant concentrations (each raised to their stoichiometric coefficients) settles to a constant value at a fixed temperature. This ratio is the equilibrium constant $K$ , and it tells you where the reaction "prefers" to sit—whether products dominate, reactants dominate, or both coexist in comparable amounts.

The crucial insight: $K$ is a thermodynamic property tied to the standard Gibbs free energy change of the reaction through

\Delta G^\circ = -RT \ln K

Because $\Delta G^\circ$ itself depends on temperature (via the temperature dependence of enthalpy and entropy), so does $K$ .

Examining the assertion

Assertion (A): For any chemical reaction at a particular temperature, the equilibrium constant is fixed and is a characteristic property.

This is true. Once you specify:

the balanced chemical equation,
the temperature,
the standard state (usually 1 bar for gases, 1 M for solutions),

the value of $K$ is determined. It does not depend on initial concentrations, the presence of a catalyst, or the size of the container. It is an intrinsic property of the reaction at that temperature.

Important

A catalyst speeds up both forward and reverse reactions equally, so equilibrium is reached faster—but the position of equilibrium (the value of $K$ ) remains unchanged.

Examining the reason

Reason (R): Equilibrium constant is independent of temperature.

This is false. The equilibrium constant is strongly temperature-dependent. The quantitative relationship is given by the van 't Hoff equation:

\frac{d \ln K}{dT} = \frac{\Delta H^\circ}{RT^2}

Integrating between two temperatures $T_1$ and $T_2$ :

\ln \frac{K_2}{K_1} = -\frac{\Delta H^\circ}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right)

What this means: …

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Q.Assertion (A): For any chemical reaction at a particular temperature, the equilibrium constant is fixed and is a characteristic property. Reason (R): Equilibrium constant is independent of temperature.

Why equilibrium constants matter

Examining the assertion

Examining the reason

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Q.Assertion (A): For any chemical reaction at a particular temperature, the equilibrium constant is fixed and is a characteristic property.
Reason (R): Equilibrium constant is independent of temperature.

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