Partial Pressures and the Equilibrium Constant

# Partial Pressures and the Equilibrium Constant - K c = K p...

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Partial Pressures and the Equilibrium Constant -for gas phase reactions the equilibrium constants can be expressed in partial pressures rather than concentrations -pressure is proportional to the concentration (gases) -deal gas law -P=MRT and M = P/RT K c = K p (1/RT) K c = K p {RT} -1 or K p = K c (RT) 1 R=0.0821 Latm/molK -relationship between K p and K c K p = K c (RT) Δn or K c = K p (RT) -Δn Δn= number of moles of gaseous products – number of moles of gaseous reactants
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Unformatted text preview: K c = K p when the number of moles stays constant (no change) Example 17-15 I x atm C-0.34xatm +0.34x atm +0.17xatm E x-0.34x 0.34x 0.17x P tot = P partial + P partial 0.25atm= x-0.34x + 0.34x+0.17x 0.25 atm = 1.17xatm x=0.21 atm Since NOBr is 34% dissociated, it is 66% undissociated...
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## This note was uploaded on 10/04/2011 for the course CHEM 1212 taught by Professor Suggs during the Spring '08 term at UGA.

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