Activation energy calculator is an essential tool designed for determining the minimum amount of energy required to start a chemical reaction. It helps scientists and researchers to speed up reactions and make chemical processes work better.

## Steps to Use Activation Energy Calculator:

If you don’t want to indulge in manual calculation and want to save your precious time, here our Arrhenius equation calculator comes in. Follow these simple steps to pursue its functioning:

**What to Enter?**

**Choose the Option:**First, choose all the parameters in which you want to calculate.**Insert values:**Enter the values into the following field:- Rate Coefficient (K)
- Temperature (T)
- Constant (A)

**What will you Get?**

**Activation Energy:**Step-by-step calculations about activation energy that occurs during a chemical reaction

## Activation Energy Formula:

Here is the formula that our activation energy calculator uses to find out the results such as:

**$$ \Large E_a = -R \times T \times \ln\left(\frac{k}{A}\right) $$**

Where,

**R**– The universal gas constant. Its value is 8.314 J/(K ⋅ mol)**T**– Represents the temperature in the surrounding environment**K**– The reaction rate coefficient**A**– Represents the frequency factor

## How to Find Activation Energy?

We will use an activation energy example of activation energy which helps you understand the __chemical__ reaction mechanism better. You can also try our activation energy calculator for this purpose.

### Example:

Imagine you're conducting a chemistry experiment where you're studying the rate of a chemical reaction. You've collected data for two different temperatures. At 25°C (298.15 K), the reaction rate constant (k) is 0.005 s⁻¹, and at 45°C (318.15 K), the reaction rate constant (k) is 0.04 s⁻¹. You know the gas constant (R) is 8.314 J/(mol·K), and you'll assume a pre-exponential factor (A) of 1000.

Using the given data, let's calculate the activation energy (E_a) for this reaction.

First, let's find the natural logarithm of the ratio $ \frac {K}{A} $:

$$ \ln\left(\frac{k}{A}\right) = \ln\left(\frac{0.04}{1000}\right) $$

$$ \ln\left(\frac{0.04}{1000}\right) \approx -5.2144\;(rounded\;to\;four\;decimal\;places) $$

Calculate the temperature difference (ΔT) between the two data points:

$$ \Delta T = 318.15 \, \text{K} - 298.15 \, \text{K} = 20 \, \text{K} $$

Now, calculate the activation energy (E_a) using the activation energy equation:

$$ E_a = -R \times \Delta T \times \ln\left(\frac{k}{A}\right) = -8.314 J/(mol·K) \times 20\, K \times \ln\left(\frac{0.04}{1000}\right) $$

$$ E_a = -8.314 \, \text{J/(mol·K)} \times 20 \, \text{K} \times (-5.2144) \approx 867.8928 \, \text{J/mol} $$

So, for this chemical reaction, the activation energy (E_a) is approximately 867.8928 Joules per __mole__.

## FAQs:

### What is the Arrhenius equation?

The Arrhenius equation is like a special formula in chemistry. It helps us figure out the relationship between temperature and reaction speed. The higher the temperature, the faster the reaction goes, and the Arrhenius equation helps us calculate that.

### What are the units for activation energy?

Activation energy is typically measured in joules per mole (J/mol) or kilojoules per mole (kJ/mol) and represented by the symbol Ea.

### Is activation energy always a positive value?

Yes, activation energy is always a positive value because it represents the energy required to start a reaction.

## References:

**Wikihow.com:** What is activation energy? Use the equation form for multiple temperatures and constants, and Plug in the given data.