# CHEM 1C Lecture Notes - Lecture 6: Reaction Quotient, Chemical Equation, Reversible Reaction

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Published on 2 Jul 2018
School
UC-Irvine
Department
Chemistry
Course
CHEM 1C
Professor
Express the overall equation using K1 and K2
Homogeneous equilibrium applies to reactions in which all reacting species are in the
same phase.
For gas phase reactions we can define an alternative equilibrium constant Kp, which is
based partial pressures instead of concentrations
P is defined in atm, but measured relative to 1 atm, so that Kp remains implicitly
dimensionless
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What is the relation between Kc and Kp?
aA (g) + bB (g) cC (g) + dD (g)
n = moles of gaseous products - moles of gaseous reactants
= (c + d) - (a + b)
Example: The equilibrium concentrations for the reaction between carbon monoxide and
molecular chlorine to form COCl2 (g) at 740C are [CO] = 0.012 M, [Cl2] = 0.054 M, and [COCl2]
= 0.14 M. Calculate the equilibrium constants Kc and Kp (R = 0.082 L atm K-1 mol-1)
Heterogeneous equilibrium applies to reactions in which reactants and products are in
different phases.
The concentration of solids and pure liquids are not included in the expression for
the equilibrium constant
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