CHEM-UA 109 Lecture Notes - Lecture 8: Chemical Equilibrium, Oxidation State, Reaction Rate

• School: New York University
• Department: Chemistry
• Course: CHEM-UA 109
• Professor: Pollock

Document Summary

In chemical reactions, the reverse and forward reactions are not always exactly the same this can be explained by le chatelier"s principle. In chemical equilibrium, it also has to be a closed system, so no reactant leaves the system. Le chatelier"s principle states that a system in equilibrium will always try to relieve stress. In the equation ch4(g) + h2o(g) 3h2o(g) + co(g), when you add more ch4, then the forward reaction will increase, and then as more products are formed, the reverse reaction rate increases, and the cycle goes on. When concentration of methane is reduced, then the rate of forward reaction decreases. Heat can be considered at a reactant/product, so it follows the same principle. There is a tendency in nature to change to a state of lower energy (enthalpy) exothermic: therefore, exothermic reactions are more likely. The tendency in nature to change to a state of greater randomness or disorder.