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The rate constant is the reaction rate divided by the concentration terms.
You need to know the rate of the reaction, as well as the concentrations of all reactants. Then you plug those values into the equation of rate = k[A][B] or whatever the rate equation happens to be.
A rate constant
The equilibrium constant can tell us how the reaction is going. If the constant is grater than one there are more products than reactants, so the reaction os closer to completion. If the equilibrium constant is less than 1 it shows that there are a lot more products than reactants so the reaction has not really started yet.
The total mass remain constant after a chemical reaction.
After it reaches equalibrium
The rate constant is the reaction rate divided by the concentration terms.
The rate constant is the reaction rate divided by the concentration terms.
The molarity of products is divided by the molarity of reactants
it's when it changes to one thing then changes to the original state
Kc is the equilibrium constant of a chemical reaction; Kp is the equilibrium constant of a chemical reaction at constant pressure.
The rates of the reaction at different temperatures are determined experimentally while the concentrations of the reactants are kept constant. The value of k is calculated for each trial.A graph is then plotted with lnk against 1/T. The activation energy (Ea) can be determined with the equation -EA=gradient of the line x the gas constant (8.31 J/K/mol).
You need to know the rate of the reaction, as well as the concentrations of all reactants. Then you plug those values into the equation of rate = k[A][B] or whatever the rate equation happens to be.
constant
A relative rate constant the rate at which a reaction will take place. Ex. V = k [A][B] the constant ,k, is a constant value for the rate of the reaction in said equation.
Kb= 1/Kf (:
Constant variables are constant, they do not change. Derived variables are not constant. They are determined by the other values in the equation.