To write the Keq for a reaction, the equilibrium concentrations of all reactants and products must be known. A specific example of this is how we define pH: the log of the equilibrium constant for any acid-base reaction. Just that simple, provided, of course, that the reaction does NOT go to 100% completion. Same principles apply to dissolution of partially soluble materials. If done correctly with consideration to chemical activity and coefficients, the so-called 'thermodynamic' equilibrium constants are obtained and are used in estimating quantities such as the entropy and enthalpy change of reaction.
The more difficult ( and interesting part ) is how do we know what those concentrations are? Mass balance equations are a good place to start along with any stoichiometric considerations...easy to stick to 1:1 electrolytes and other simple reactions.
If you continuously add reactants even after the reaction has attained the equilibrium then according to Le Chatelier's principle, the reaction will again proceed in forward direction in order to neutralise the reactants and once again the attain the state of equilibrium.
A rate constant
Many chemical reactions, like combustion , go to completion and not to equilibrium. It is normally desirable to give a chemical reaction time to reach equilibrium in order you get the maximum yield of one or more products.
In a zero order overall process, the rate and rate constant will be the same. (Reaction order is an exponent, and if that exponent is "0" then the value is "1" and will cancel out.)
In order to bring the system to equilibrium, action and reaction cancel out. The resultant is the reaction.
The reaction rate depends on the order of the reaction. In general (except for zero order), as the reaction progresses, the rate decreases with time.
The rate constant include all parameters ((but not concentration) affecting the rate of a chemical reaction.The expression "specific reaction rate" is used when the molar concentration of reactants is a unit.
order is 0
It depends on the order of the reaction. If it is zero order, decreasing the reactant concentration will have NO effect on the rate. If it is 1st or 2nd order (or more), then decreasing the concentration will DECREASE the reaction rate.
Since the reaction is first-order, the half-life is constant and equals ln(2)/k, and the units of k are s-1. In this case, the half-life is ln(2)/(.0000739 s-1) = 9379.529 seconds.
If a forward and reverse reaction happen at the same rate, the result is called a dynamic equilibrium; the overall chemical composition does not change, even though reactions are constantly taking place.
Collision theory is when mollecules must collide with one another in order to cause a reaction. In a succesful collision, old bonds are broken as new bonds are formed. Equilibrium is a state in which forces cancel one another.