CHM 104 1st Edition Lecture 9 Outline of Last Lecture I Chemical Equilibria Outline of Current Lecture II Kc versus Kp III Heterogeneous equilibria IV Equilibrium Calculations Current Lecture Kc versus Kp Heterogeneous Equilibrium Equilibrium equation can be written using molarity or partial pressures gases This can change K Pressure of the gas is proportional to molarity PV nRT P n v RT P eq RT Example 2NO2 g N2O4 g In General aA bBcC dD If c d a b 0 Kp Kc RT c d a b Kp Kc All are concentrations AFTER an equilibrium has been established These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute Pure solids and liquids are replaced by 1 s their concentrations DON T depend on the container volume just the density of the substance Equilibrium Calculations K can be calculated if ALL equilibrium concentrations are known Example CO g H2O g CO2 g H2 g CO eq 0 0100 M H2O eq 0 0050 M CO2 eq 0 100 M H2 eq 0 200 M If K is known then eq can be determined Equilibrium concentrations are not the same in 2 examples b but both satisfy the Mass Action Equation Often it is convenient to summarize changes in an ICE table 2CH4 C2H2 3H2 I 0 100 M 0 0 C 2 0 035 0 035 3 0 035 E 0 45 0 035 0 105
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