Chemical Reactions And Equilibrium - Chemistry Assignment Help

Assignment Task

Introduction

In many chemical reactions, reactants are not completely converted to products. Instead, the reaction goes to some steady state in which the concentrations of both products and reactants do not change over time. The reaction is said to be at equilibrium. At this point in the reaction, the rate of the forward reaction and the rate of the reverse reaction are equal. The system has reached a dynamic equilibrium in which the chemical conversion is still occurring, but at an equal rate in both the forward and reverse reaction. For example, consider the following reaction:

aA + bB ? cC + dD

whereA,B,C,andDindicatereactantsandproducts;a,b,c,andd arecoefficientsinthebalanced chemical equation; and the double arrow (?)indicates the reaction can proceed in either direction. The equilibrium constant expression for a reaction is obtained by raising each molar concentration term to a power equalto the coefficient in thechemicalreaction,multiplyingthe molarconcentrationsofthe products,anddividingbytheproductofthemolarconcentrations ofthereactants.Theequilibrium constant, K, is the value obtained in the equilibrium constant expression when equilibrium concentrationsareplacedintheexpression.Thevalue of Kisaconstantforaparticularreactionata certaintemperature.Thismeansthatifarbitrary quantitiesofA,B,C,andDaremixed,thereactionwill proceeduntilthenumericalvalues of the concentrations of the sespecies satisfy the equation. For the example described,the equilibrium constant expression has the form.

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