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2. Reaction rate - Wikipedia

   en.wikipedia.org/wiki/Reaction_rate

   Iron rusting has a low reaction rate. This process is slow. Wood combustion has a high reaction rate. This process is fast. The reaction rate or rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time. [1]

3. Law of mass action - Wikipedia

   en.wikipedia.org/wiki/Law_of_mass_action

   Guldberg and Waage also recognized that chemical equilibrium is a dynamic process in which rates of reaction for the forward and backward reactions must be equal at chemical equilibrium. In order to derive the expression of the equilibrium constant appealing to kinetics, the expression of the rate equation must be used.

4. Reaction rate constant - Wikipedia

   en.wikipedia.org/wiki/Reaction_rate_constant

   where A and B are reactants C is a product a, b, and c are stoichiometric coefficients,. the reaction rate is often found to have the form: = [] [] Here ⁠ ⁠ is the reaction rate constant that depends on temperature, and [A] and [B] are the molar concentrations of substances A and B in moles per unit volume of solution, assuming the reaction is taking place throughout the volume of the ...

5. Rate equation - Wikipedia

   en.wikipedia.org/wiki/Rate_equation

   A common form for the rate equation is a power law: [6] = [] [] The constant ⁠ ⁠ is called the rate constant.The exponents, which can be fractional, [6] are called partial orders of reaction and their sum is the overall order of reaction.

6. Arrhenius equation - Wikipedia

   en.wikipedia.org/wiki/Arrhenius_equation

   This has the same form as an equation for a straight line: = +, where x is the reciprocal of T. So, when a reaction has a rate constant obeying the Arrhenius equation, a plot of ln k versus T −1 gives a straight line, whose slope and intercept can be used to determine E a and A respectively. This procedure is common in experimental chemical ...

7. Chemical reaction - Wikipedia

   en.wikipedia.org/wiki/Chemical_reaction

   Different chemical reactions are used during chemical synthesis in order to obtain the desired product. In biochemistry, a consecutive series of chemical reactions (where the product of one reaction is the reactant of the next reaction) form metabolic pathways. These reactions are often catalyzed by protein enzymes.

8. Chemical kinetics - Wikipedia

   en.wikipedia.org/wiki/Chemical_kinetics

   Chemical kinetics, also known as reaction kinetics, is the branch of physical chemistry that is concerned with understanding the rates of chemical reactions. It is different from chemical thermodynamics , which deals with the direction in which a reaction occurs but in itself tells nothing about its rate.

9. Activation energy - Wikipedia

   en.wikipedia.org/wiki/Activation_energy

   In the Arrhenius model of reaction rates, activation energy is the minimum amount of energy that must be available to reactants for a chemical reaction to occur. [1] The activation energy ( E a ) of a reaction is measured in kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol). [ 2 ]