We always struggled to serve you with the best online calculations, thus, there's a humble request to either disable the AD blocker or go with premium plans to use the AD-Free version for calculators.
Disable your Adblocker and refresh your web page 😊
Table of Content
The activation energy calculator helps you in calculating activation energy to initiate a chemical reaction. Just enter the necessary inputs and the tool will readily show results, with the steps shown.
“It is the minimum energy required for a chemical reaction to occur”
Due to the activation energy, the atoms of the reactants undergo bond breakage and hence the reaction starts this way.
If you are willing to calculate the energy by hand, you need to understand the Arrhenius equation as follows:
E_a = -R * T * ln(k / A)
You can visit here to explore the activation energy graph if your goal comes up with calculations through it.
How to find activation energy with temperature and rate constant as follows:
Temperature = 253 K
Frequency factor = A = 210
Rate Constant = 100
E_a = -R * T * ln(k / A)
E_a = -0.008314 * 373.15 * ln(100 / 1000)
E_a = (-3.1023691) * (ln(0.1))
E_a = (-3.1023691) * (-2.302585092994)
E_a = 7.143 KJ
Our calculator also computes the same answer but reduces the times from minutes to milliseconds. The tool maintains accuracy in calculations and shows complete steps that are involved in calculating activation energy.
To do this, follow the key points:
To use the calculator, you need to stick to the following guide:
Sometimes, a limiting reagent also affects the reaction kinematics and hence the activation energy also shows deviation.
Yes, it does! As there is an inverse relation between both quantities, increasing activation energy will decrease the rate of the reaction. However, our activation energy calculator helps you to estimate the minimum energy that you may require to start a reaction according to the situations given.
Yes! Enzymes always tend to increase the reaction rate by lowering the activation energy. Basically, enzymes use their active sites to bind molecules of the substrates. In this way, they reduce the requirement of activation energy at higher rates.
Yes, of course! Basically, the activation energy is not dependent upon temperature and rate, but a slower rate due to higher temperature tends the energy to be negative. This can also be calculated through an activation energy calculator without any hassle.
The activation energy of a chemical reaction is only dependent on the nature of the chemical species in that particular reaction:
From the source Wikipedia: Activation energy, Temperature dependence and the relation to the Arrhenius equation, Catalysts, Relationship with Gibbs energy of activation, Negative activation energy, Activation energy in a 2D potential energy surface
From the source Lumen Learning: Activation Energy and the Arrhenius Equation, Determining the Activation Energy, Reaction Mechanisms