Chemical Equilibrium I

This General Chemistry lecture introduces the concept of chemical equilibrium. We describe the dependence of the Gibbs Free Energy on pressure and concentration, and derive the existence of the equilibrium constant for a reaction. Using the dimerization of nitrogen dioxide as an example, we show how to calculate the equilibrium partial pressures or concentrations for any reaction from any initial conditions using thermodynamic data.

Category:

Education

Tags:

• chemistry
• General Chemistry
• equilibrium
• enthalpy
• entropy
• Gibbs Free Energy
• pressure
• concentration

[chemdog8]

@bomberfun1 Hi. This term represents the reactant pressure (N2O4) at equilibrium, so it belongs in the denominator as shown. The way to interpret the expression is that the initial pressure of N2O4 was 1 bar, but some of it reacted to form NO2. The final equilibrium pressure of N2O4 is 1-0.5PNO2) because for every mole of NO2 formed in the reaction, only 0.5 moles of N2O4 disappears.

[ajc31sacount]

Your lesson was very helpfull. However, i was just wonder about if the equilibrium was on top of the chuck then it wouldn't do the same face results as the poofular mechanics. If this is so, then what results would toder have?

[shannonelise4989]

thank you for your lessons