1.
Chemical Equilibrium: the state where the concentrations of all reactants and products remain constant with time.
2.
Equilibrium Constant: symbol is "K" from the equilibrium expression. The greater the value for K, the more tendency the reaction to go in the forward direction. (the equilibrium is to the right/products are favored)
3.
Equilibrium Expression: symbol is "K" from the equilibrium expression. The greater the value for K, the more tendency the reaction to go in the forward direction. (the equilibrium is to the right/products are favored)
4.
Equilibrium Position: a set of equilibrium concentrations
5.
Heterogeneous Equilibria: system where there is more than one phase present
6.
Homogeneous Equilibria: systems where all of the phases are the same (usually gas phases)
7.
Law of Mass Action: proposed by Guldberg and Waage in 1864; a general description of the equilibrium constant; it defines the equilibrium constant expression.
8.
LeChatelier's Principle: states that if a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change.
9.
Reaction Quotient Q: is calculated using the law of mass action using initial concentrations; then is compared to actual K value to see where equilibrium would shift.
10.
The Haber Process: a process form making ammonia using the reaction. N2(g) + 3H2(g) → 2NH3(g)
