JEE Main Deleted Syllabus 2025: Reduced Chapters & Topics PCM

Equilibrium - Practice Questions & MCQ

Edited By admin | Updated on Sep 18, 2023 18:35 AM | #JEE Main

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13 Questions around this concept.

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The equilibrium constant at 298 K for a reaction A+BC+D is 100. If the initial concentration of all the four species were 1 M each, then equilibrium concentration of D (in mol L⁻¹) will be :

0.182

0.818

1.818

1.182

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Concepts Covered - 2

Introduction to chemical equilibrium

The word "equilibrium" in a physical sense is explained as the "No change of state of the body". When the two opposing processes (reaction) occur simultaneously with equal rates, the system is in a state of equilibrium. Equilibrium is classified as follows

When an equilibrium exists between the same chemical species, it is called physical equilibrium. For example:
$\mathrm{H_{2}O(s)\: \rightleftharpoons \: H_{2}O(l)}$

When an equilibrium exists between different chemical species, it is called chemical equilibrium.
$\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{g})$

If a chemical equilibrium has only one phase, it is called homogenous, and if more than one phase it is called heterogeneous.

Chemical Equilibrium
"It is the state of a reversible reaction at which measurable properties like colour, density, pressure concentration are nearly unchangeable.

Here V₁ and V₂ are the rates of forward and backward reactions respectively. i.e, equilibrium is the state in a reversible reaction at which the rate of forward and backward reactions or two opposing reactions are the same.

Types of reactions
Chemical reactions are of two types:
Irreversible Reaction: Such reactions occur in one direction only and get completed.
For example:
(i) When unreactive products or solid products are formed.

$\mathrm{NH}_{4} \mathrm{NO}_{2} \stackrel{\Delta}{\longrightarrow} \mathrm{N}_{2}+2 \mathrm{H}_{2} \mathrm{O}$

(ii) All precipitate reactions are irreversible.

$\begin{array}{l}{\mathrm{BaCl}_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{BaSO}_{4}+2 \mathrm{HCl}} \\ {\text { aq. } \quad \: \: \: \: \text { aq. } \quad \: \: \: \: \: \: \: \: \: \mathrm{ppt.} \quad\: \: \: \: \text { aq. }}\end{array}$

(iii) Neutralisation reactions are also irreversible.

$\mathrm{H}_{2} \mathrm{SO}_{4}+2 \mathrm{KOH} \rightarrow \mathrm{K}_{2} \mathrm{SO}_{4}+2 \mathrm{H}_{2} \mathrm{O}$

(iv) Redox reactions are also irreversible.

$2 \mathrm{FeCl}_{3}+\mathrm{SnCl}_{2} \rightarrow \mathrm{SnCl}_{4}+2 \mathrm{FeCl}_{2}$

(v) Combustion reactions are also irreversible.

$2 \mathrm{Mg}+\mathrm{O}_{2} \rightarrow 2 \mathrm{MgO}$

Reversible Reactions: Such reactions occur in both directions i.e., forward and backward direction however never complete as the products can give back the reactants under same or different conditions. For example:

$\mathrm{N}_{2}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO}$

Vapourization of water in open flask is irreversible reaction while in closed flask it is reversible.
Decomposition of CaCO₃in open flask is irreversible reaction while in closed flask it is reversible.

Characteristics of Chemical Equilibrium

The following are the important characteristics of equilibrium:

It is obtained only when the reversible reaction is carried out in a closed space.
Here the rate of forward reaction is equal to the rate of backward reaction.
Here both forward and backward reactions are taking place at the same rate hence the relative amounts of the reactants and products present at equilibrium do not change with time.
At constant temperature, it is characterized by properties like color, density, pressure, etc.
It is possible from both sides.
It is dynamic in nature. It means the reaction or process is not going to be ceased as the reaction occurs in both directions with equal rates.
A catalyst cannot alter the positive of equilibrium as it accelerates both the forward and backward reactions to the same extent this means the same state of equilibrium is reaction i.e., a positive catalyst can set up equilibrium in less time but can not change it.
At equilibrium $\Delta$ G is equal to zero i.e.,
$\Delta$ G = $\Delta$ H - T $\Delta$ S
So,
$\Delta$ H = T $\Delta$ S
Under similar conditions of temperature, concentration, and pressure, the same state of equilibrium is reached.