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`E_a = R*(ln(k_2/k_1))/(1/T_1 -1/T_2)`

Enter a value for all fields

The **Arrhenius Activation Energy for Two Temperature **calculator uses the Arrhenius equation to compute activation energy based on two temperatures and two reaction rate constants.

**INSTRUCTIONS:** Choose units and enter the following:

- (
**k**) Reaction rate constant 1_{1} - (
**k**Reaction rate constant 2_{2}) - (
**T**) Temperature 1_{1} - (
**T**) Temperature 2_{2}

**Activation Energy(E _{a}): **The calculator returns the activation energy in Joules per mole.

The Arrhenius Equation is used to describe the temperature dependence of reaction rates in chemical reactions. It was developed by Swedish chemist Svante Arrhenius in the late 19th century. The Arrhenius Equation is particularly relevant in the field of chemical kinetics, which studies the speed or rate at which chemical reactions occur.

The **Arrhenius Equation**, `k = A*e^(-E_a/"RT")`, can be rewritten (as shown below) to show the change from k_{1} to k_{2} when a temperature change from T_{1} to T_{2} takes place.

The Activation Energy equation using the Arrhenius formula is:

`E_a = R*(ln(k_2/k_1))/(1/T_1 -1/T_2)`

where:

- E
_{a}is the activation energy in Joules per mole (J/mol) - k
_{1}is the reaction rate constant at temperature 1 - k
_{2}is the reaction rate constant at temperature 2 - R is the ideal gas constant (8.314 J/mol*K)
- T
_{1}is temperature 1 in Kelvin (K) - T
_{2}is temperature 2 in Kelvin (K)

The calculator converts both temperatures to Kelvin so they cancel out properly.

- Arrhenius Equation (for two temperatures)
- Ideal Gas Constant (R)
- Arrhenius Equation
- Temperature Coefficient Q10

Whitten, et al. "Chemistry" 10th Edition. Pp. 645