Determine the value of equilibrium constant (KC. ) for the reaction A2( g)+B2( g) ⇌2 AB(g) If 10

step 1 In this problem, we have to determine the value of equilibrium constant KC for the reaction. A2

Determine the value of equilibrium constant (KC. ) for the...

Determine the value of equilibrium constant $\left(\mathrm{K}_{\mathrm{C}}\right.$ ) for the reaction $$ \mathrm{A}_{2}(\mathrm{~g})+\mathrm{B}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g}) $$ If 10 moles of $A_{2} ; 15$ moles of $B_{2}$ and 5 moles of $A B$ are placed in a 2 litre vessel and allowed to come to equilibrium. The final concentration of $\mathrm{AB}$ is $7.5 \mathrm{M}$ : (a) $4.5$ (b) $1.5$ (c) $0.6$ (d) None of these

Determine the value of equilibrium constant $\left(\mathrm{K}_{\mathrm{C}}\right.$ ) for the reaction
$$
\mathrm{A}_{2}(\mathrm{~g})+\mathrm{B}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AB}(\mathrm{g})
$$
If 10 moles of $A_{2} ; 15$ moles of $B_{2}$ and 5 moles of $A B$ are placed in a 2 litre vessel and allowed to come to equilibrium. The final concentration of $\mathrm{AB}$ is $7.5 \mathrm{M}$ :
(a) $4.5$
(b) $1.5$
(c) $0.6$
(d) None of these

Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in which the rates of the forward and reverse reactions are equal, causing the concentrations of the reactants and products to remain constant over time. Despite ongoing reactions, the net change in concentration is zero, and the system is dynamic with continual microscopic reversibility.

Equilibrium Constant (Kc)

The equilibrium constant, denoted as Kc, quantifies the ratio of the concentrations of products to reactants at equilibrium, with each concentration raised to the power of its stoichiometric coefficient. It provides a measure of the extent to which a reaction proceeds and is specific to a given reaction at a particular temperature.

ICE Table Method

The ICE table (Initial, Change, Equilibrium) is a systematic approach used in chemistry to track the concentration changes of reactants and products over the course of a reaction as it approaches equilibrium. By setting up an ICE table, one can easily calculate unknown equilibrium concentrations and, consequently, the equilibrium constant.

Stoichiometric Relationships

Stoichiometric relationships refer to the quantitative relationships between reactants and products as indicated by the balanced chemical equation. These relationships are crucial for determining how changes in the amount of one substance affect the amounts of others, thereby allowing for the correct setup of equilibrium calculations.

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