What is the equilibrium concentration of each of the...

What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of $\mathrm{ICl}$ was $0.78 \mathrm{M}$ ? $2 \mathrm{ICl}(\mathrm{g}) \rightleftharpoons \mathrm{I}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) ; \quad K_{\mathrm{c}}=0.14$

Key Concepts

Stoichiometry in Equilibrium Calculations

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In equilibrium calculations, it is crucial for relating the changes in concentration of one species to the changes in others, based on the balanced equation. This allows for the proper setup of expressions and equations to solve for unknown concentrations at equilibrium.

ICE Table Method

The ICE (Initial, Change, Equilibrium) table is an organized method used for calculating the changes in concentrations of chemicals as a reaction reaches equilibrium. The approach involves listing the initial concentrations, determining the changes that occur as the system reaches equilibrium based on the stoichiometry of the reaction, and then calculating the equilibrium concentrations.

Equilibrium Constant (Kc) Expression

The equilibrium constant, represented as Kc when concentrations are used, is defined by the ratio of the products of the equilibrium concentrations of products raised to their stoichiometric coefficients over the products of the equilibrium concentrations of reactants raised to their stoichiometric coefficients. It quantifies the extent to which a reaction proceeds and is a key tool in predicting the direction of the reaction.

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products over time. This concept is fundamental to understanding how reactions balance and how changes in conditions affect the concentrations of the species involved.

Transcript

00:01 So the question is what is the equilibrium concentration of each of the substance in the equilibrium when the initial concentration of icl was 0 .78 molar and the reaction is given to icl gases give i2 gaseous plus cl2 gaseous where kc is given 0 .14.

00:23 So first we should know what is initial concentration, what is equilibrium concentration and what is kc.

00:34 Kc is actually the equilibrium constant.

00:40 It is called the equilibrium constant with respect to the molar concentration of the gaseous mixture.

00:45 So kc is written as this is the kc formula for the reaction of i2 plus c.

00:54 Cl2 gives icl where first the concentration of products are written which is divided by the concentration of reactant and they are raised to the power of their stoichiometric coefficient because here the stoichiometric coefficient is 2 so it is raised to the power of 2 so we know initial concentration means when the reaction started so they have given the initial concentration of icl as 0 .78 molar which is the reactant so this was the initial concentration whereas the initial concentration when product was not formed so their initial concentration will be 0 both of i2 and cl 2 this we know now we have to find out the equilibrium concentration when both the reactor and products were in equilibrium so we have to assume let the equilibrium concentration of i 2 i2 and cl 2 we have assumed as x and x whereas the concentration of icel will be 0 .78 minus 2x because in initial was 0 .78 then equilibrium concentration will be 0 .78 minus 2x because both the products are taken as x.

02:10 Now we'll put the values in casey formula.

02:16 So after putting the value of case is 0 .14 and i2 and cl2 as x and x and i .l 2 as 0...

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