# How is EA slope calculated?

## What is EA in chemistry?

The activation energy (Ea) is the minimum amount of the extra energy absorbed by the reactant molecules from an energy source such as heat, light, etc., to attain the threshold value for effective collisions to occur and thereby to form an intermediate complex (active state) that finally results in product formation.

## How do you calculate activation energy?

1. Step 1: Convert temperatures from degrees Celsius to Kelvin. T = degrees Celsius + 273.15. T1 = 3 + 273.15.
2. Step 2 – Find Ea ln(k2/k1) = Ea/R x (1/T1 – 1/T2)
3. Answer: The activation energy for this reaction is 4.59 x 104 J/mol or 45.9 kJ/mol.

## What is the EA activation energy and how is it calculated?

The value of the slope (m) is equal to -Ea/R where R is a constant equal to 8.314 J/mol-K. The activation energy can also be found algebraically by substituting two rate constants (k1, k2) and the two corresponding reaction temperatures (T1, T2) into the Arrhenius Equation (2).

## What is activation energy units?

What is the SI Unit of Activation Energy? Activation energy is denoted by Ea. It is usually measured in joules (J) and or kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).

## What is k in Arrhenius equation?

In the Arrhenius equation, k is the reaction-rate constant, A represents the frequency at which atoms and molecules collide in a way that leads to a reaction, E is the activation energy for the reaction, R is the ideal gas constant (8.314 joules per kelvin per mole), and T is the absolute temperature.

## What is AE in Arrhenius equation?

The Arrhenius equation is k = Ae^(-Ea/RT), where A is the frequency or pre-exponential factor and e^(-Ea/RT) represents the fraction of collisions that have enough energy to overcome the activation barrier (i.e., have energy greater than or equal to the activation energy Ea) at temperature T.

## What is activation energy examples?

This energy is called activation energy. For example, activation energy is needed to start a car engine. Turning the key causes a spark that activates the burning of gasoline in the engine. The combustion of gas won’t occur without the spark of energy to begin the reaction.

## How does k relate to activation energy?

The Arrhenius equation is k=Ae−Ea/RT. A minimum energy (activation energy,vEa) is required for a collision between molecules to result in a chemical reaction. Plots of potential energy for a system versus the reaction coordinate show an energy barrier that must be overcome for the reaction to occur.

## What is Arrhenius equation How does it help in calculating the activation energy?

The Arrhenius equation allows us to calculate activation energies if the rate constant is known, or vice versa. As well, it mathematically expresses the relationships we established earlier: as activation energy term Ea increases, the rate constant k decreases and therefore the rate of reaction decreases.

## What is k in k AE EA RT?

k = Ae. −Ea. RT. Both A and Ea are specific to a given reaction. k is the rate constant.

## What is the activation energy of a chemical reaction quizlet?

Activation energy is the energy absorbed before it can start a chemical reaction.

## What is the activation energy quizlet?

activation energy. The amount of energy required to cause a chemical reaction;specifically the energy required to reach the transition state.

## What is activation energy Ev?

Activation Energy , usually denoted by its symbol Ea, is defined as the minimum amount of energy required to initiate a particular process. It is usually used in the context of chemical reactions, i.e., as the minimum amount of energy that chemical reactants must possess before they can undergo a chemical reaction.

## Where is the activation energy located?

The source of activation energy is typically heat, with reactant molecules absorbing thermal energy from their surroundings.

## How can you graphically find the activation energy of the reaction?

1. Slope = -Ea2.303R.
2. or -Ea = -5841 x 2.303 x 8.314.
3. Ea = 111838.45 J mol-1 = 111.838 kJ mol-1

## How do you find the rate constant k?

(It’s also the easiest method for zero-order reactions since the rate of the reaction is equal to the rate constant!) The dependence of the rate constant on temperature is well defined by the Arrhenius equation: k = A * exp(-E /(R * T)) .