401ChemEqbm

401ChemEqbm - Chemical Equilibrium Chapters 15 and 18...

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Lesson 16 1 Lesson 16 Chemical Equilibrium Chapters 15 and 18 (Petrucci et al., 9 th Ed.) Lesson 16 The nature of chemical equilibrium • Consider the following reversible reaction CO ( g ) + 2 H 2 ( g ) → CH 3 OH ( g ) CH 3 OH ( g ) → CO ( g ) + 2 H 2 ( g ) • When chemical equilibrium is reached, the concentrations of all reactants and products remain constant • Chemical equilibrium is a dynamic process: When it is reached, the rate of the forward reaction equals the rate of the reverse reaction the reaction does not stop Lesson 16 CO ( g ) + 2 H 2 ( g ) = CH 3 OH ( g )
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Lesson 16 2 Lesson 16 Lesson 16 The equilibrium constant K c For the reaction CO( g ) + 2 H 2 ( g ) = CH 3 OH( g ) the equilibrium constant is defined as: Using the values given in Table 15.1: 2 2 3 ] ][ [ ] [ H CO OH CH K c 5 . 14 ) 176 . 0 )( 138 . 0 ( ) 062 . 0 ( ) 151 . 0 )( 0753 . 0 ( ) 0247 . 0 ( ) 0822 . 0 )( 0911 . 0 ( ) 00892 . 0 ( 2 2 2 c K The value of the equilibrium constant is constant at a given temperature Lesson 16 Chemical equilibrium is reversible and spontaneous CO( g ) + 2 H 2 ( g ) = CH 3 OH( g ) What happens if we add more CO ( g ) after chemical equilibrium is reached? – [CO] > [CO] eq – Rate of forward reaction > Rate of reverse reaction – More CH 3 OH is formed → [CH 3 OH] increases → rate of reverse reaction increases
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This note was uploaded on 11/29/2011 for the course CHE 102 taught by Professor Simon during the Fall '08 term at Waterloo.

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401ChemEqbm - Chemical Equilibrium Chapters 15 and 18...

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