Temperature is considered a major factor that affects the rate of a chemical reaction. It is considered a source of energy in order to have a chemical reaction occur. Svante Arrhenius, a Swedish chemist, believed that the reactants in a chemical reaction needed to gain a small amount of energy in order to become products. He called this type of energy the Activation Energy. The amount of energy used in the reaction is known to be greater than the activation energy in the reaction. Arrhenius came up with an equation that demonstrated that rate constants of different kinds of chemical reactions varied with temperature. This equation indicates a rate constant that has a proportional relationship with temperature. For example, as the rate constant increases, the temperature of the chemical reaction generally also increases. As we derive Arrhenius' rate constant expression twice, the result is:
ln k2/k1= Ea/R (1/T1-1/T2)
This equation is known as Arrhenius' equation. T1 and T2 are temperature variables expressed in Kelvin. T1 can be expressed as the initial or lower temperature of the reaction, while T2 is the final or higher temperature of the reaction. Rate constants, k1 and k2, are values at T1 and T2. Ea is the activation energy expressed (Joules/mole)=(J/mol). R is the gas constant expressed as 8.3145 (Joules/mole x Kelvin)=(J/mol*K)
Some may ask how the temperature actually affects the chemical reaction rate. The answer to this is that this phenomenon is related to the collision theory. Molecules will only react if they have a sufficient amount of energy in order for a reaction to take place. When the temperature of a solution increases, the molecular energy levels will also increase which causes the reaction to go faster.
The graph of ln K vs. 1/T is a straight line. This straight line allows us to calculate the activation energy needed for the reaction.
Some interesting examples:
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