In the heterogeneous equilibrium A(s) ⇌2 B( g)+ 3 C(g). If conc. of C at equilibrium is doubled

step 1 In this problem we have given a heterogeneous equilibrium in which a solid reacts reversively to

In the heterogeneous equilibrium A(s) ⇌2 B( g)+ 3 C(g). If...

In the heterogeneous equilibrium $\mathrm{A}(\mathrm{s}) \rightleftharpoons 2 \mathrm{~B}(\mathrm{~g})+$ $3 \mathrm{C}(\mathrm{g})$. If conc. of C at equilibrium is doubled, then after the equilibrium is re- established, the conc. of B will be $\left(\frac{1}{r}\right)$ times its original value. The value of $r^2$ is

Key Concepts

Equilibrium Constant

The equilibrium constant (K) is a value that expresses the ratio of the concentrations or partial pressures of products to reactants at equilibrium, raised to the power of their respective stoichiometric coefficients. It remains constant at a given temperature and is used to quantify the position of equilibrium in chemical reactions, allowing predictions about how changes in concentration (or pressure) will affect the reaction state.

Heterogeneous Equilibrium

Heterogeneous equilibrium refers to a chemical equilibrium involving species in more than one phase, typically including solids, liquids, and gases. In such equilibria, the concentration of pure solids and liquids remain constant and do not appear in the equilibrium constant expression. This simplifies the analysis by focusing on the species whose concentrations vary, such as gases or solutes in solution.

Le Chatelier's Principle

Le Chatelier's Principle is a fundamental concept in chemical equilibrium which states that if a system at equilibrium is disturbed by changing the conditions—such as concentration, temperature, or pressure—the system will adjust itself to counteract the change and re-establish a new equilibrium. It is crucial for predicting the direction in which the reaction will shift when external changes are imposed.

Effect of Concentration Changes on Equilibrium

When the concentration of a reactant or product in a chemical equilibrium is changed, the system will shift its equilibrium position to partially counteract the imposed change, often predicted by Le Chatelier's Principle. The extent of this shift is governed by the stoichiometry of the reaction as expressed in the equilibrium constant, which helps in determining how the concentrations of other species in the system will adjust to re-establish equilibrium.

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