Arrhenius Equation Calculator is quite user-friendly tool that required input fields to get the accurate output easily. All you need to do is enter Arrhenius constant, activation energy, temperature and tap on the calculate button to get the rate constant quickly. Make your calculations easy with this free tool.
Arrhenius Equation Calculator: Arrhenius Equation is useful to know how the rate of reaction changes by changing the temperature. Calculate the rate of reaction for small molecules can be difficult and you will get this Arrhenius Equation Calculator to understand the concept. We are also giving the steps to find the reaction rate, Arrhenius Equation formula, activation energy meaning and other details.
Check out the simple steps to calculate the reaction rate using the Arrhenius Equation.
The Arrhenius equation explains how the rate of a reaction varied based on the temperature or rate constant. The general formula of the Arrhenius equation is along the lines.
k = A x e(-Ea/(kB x T))
k is the rate constant
A is the pre-exponential factor of Arrhenius constant
Ea is the activation energy
R is the universal gas constant i.e 8.314 J/K mol
T is the temperature
We know that the Arrhenius equation defines the relationship between the rate constant and temperature. The multiplication of universal gas constant, temperature defines the energy of the molecules. Dividing activation energy by the products gives the number of collisions that occur with sufficient energy to overcome the activation energy requirements. The activation energy is inversely proportional to the number of successful collisions.
When the reaction temperature increases, the number of successful collisions also increases exponentially. The Arrhenius equation deals with the substance on a per mole basis. The exponential Arrhenius equation is k = A x e(-Ea/(kB x T)).
The Arrhenius equation in logarithamic form is given here:
ln(k) = (-E/R)*(1/T) + ln(A)
Question: The activation energy of a chemical reaction is 100 kJ/mol and its factor is 10 1/Ms. Find the rate constant of this equation at a temperature of 300 K.
Activation energy Ea = 100 kJ/mol = 100000 J/mol
Arrhenius constant A = 10 1/Ms
Temperature T = 300 K
Arrhenius equation is k = A x e(-Ea/(kB x T))
k = 10 x e(-100000/(8.314 x 300)
= 10 x e(-100000/(2494.2)
= 10 x e-40.09
= 10 x 3.882 x 10-18
= 3.882 x 10-17
Therefore, the reaction rate is 3.882 x 10-17 1/Ms.
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1. What is kB is Arrhenius Equation?
Arrhenius Equation is k = A x e(-Ea/(kB x T)). Here, kB is the Boltzmann constant and its value is 1.380649 x 10-23 J/K.
2. What is the importance of the Arrhenius Equation?
The Arrhenius Equation importance is provided here:
3. What are the real-life examples of the Arrhenius Equation?
Some of the real-life examples are milk turns sour faster when kept in room temperature instead of keeping in the refrigerator, butter goes rancid faster in the summer than in the winter, eggs hard-boil much faster at sea level compared to the mountains.
4. How to find the Arrhenius Equation?
Check the Arrhenius constant, activation energy, and temperature. Multiply the Boltzmann constant with the temperature and divide the negative of activation energy by the product. Find the exponential of the result and multiply it with the constant to check the rate constant value.