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Activation Energy for Zero Order Reactions Calculator

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✖The temperature of Gas is the measure of hotness or coldness of a gas.ⓘ Temperature of Gas [T_gas]			+10% -10%
✖The Frequency Factor from Arrhenius Equation is also known as the pre-exponential factor and it describes the frequency of reaction and correct molecular orientation.ⓘ Frequency Factor from Arrhenius Equation [A]			+10% -10%
✖The Rate Constant of Zero Order Reaction is equal to the rate of the reaction because in a zero-order reaction the rate of reaction is proportional to zero power of the concentration of the reactant.ⓘ Rate Constant of Zero Order Reaction [k]			+10% -10%

✖The Energy of Activation is the minimum amount of energy that is required to activate atoms or molecules.ⓘ Activation Energy for Zero Order Reactions [E_a]

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Activation Energy for Zero Order Reactions Solution

STEP 0: Pre-Calculation Summary

Formula Used

Energy of Activation = [R]*Temperature of Gas*(ln(Frequency Factor from Arrhenius Equation)-ln(Rate Constant of Zero Order Reaction))
E_a = [R]*T_gas*(ln(A)-ln(k))
This formula uses 1 Constants, 1 Functions, 4 Variables

Constants Used

[R] - Universal gas constant Value Taken As 8.31446261815324

Functions Used

ln - The natural logarithm, also known as the logarithm to the base e, is the inverse function of the natural exponential function., ln(Number)

Variables Used

Energy of Activation - (Measured in Joule Per Mole) - The Energy of Activation is the minimum amount of energy that is required to activate atoms or molecules.
Temperature of Gas - (Measured in Kelvin) - The temperature of Gas is the measure of hotness or coldness of a gas.
Frequency Factor from Arrhenius Equation - (Measured in Cubic Meter per Mole Second) - The Frequency Factor from Arrhenius Equation is also known as the pre-exponential factor and it describes the frequency of reaction and correct molecular orientation.
Rate Constant of Zero Order Reaction - (Measured in Mole per Cubic Meter Second) - The Rate Constant of Zero Order Reaction is equal to the rate of the reaction because in a zero-order reaction the rate of reaction is proportional to zero power of the concentration of the reactant.

STEP 1: Convert Input(s) to Base Unit

Temperature of Gas: 273 Kelvin --> 273 Kelvin No Conversion Required
Frequency Factor from Arrhenius Equation: 149000000000 Liter per Mole Second --> 149000000 Cubic Meter per Mole Second (Check conversion here)
Rate Constant of Zero Order Reaction: 0.25 Mole per Liter Second --> 250 Mole per Cubic Meter Second (Check conversion here)

STEP 2: Evaluate Formula

Substituting Input Values in Formula

E_a = [R]*T_gas*(ln(A)-ln(k)) --> [R]*273*(ln(149000000)-ln(250))

Evaluating ... ...

E_a = 30184.4334218059

STEP 3: Convert Result to Output's Unit

30184.4334218059 Joule Per Mole --> No Conversion Required

FINAL ANSWER

30184.4334218059 ≈ 30184.43 Joule Per Mole <-- Energy of Activation

(Calculation completed in 00.004 seconds)

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< Zero Order Reaction Calculators

Initial Concentration of Zero Order Reaction

LaTeX Go Initial Concentration for Zero Order Reaction = (Rate Constant of Zero Order Reaction*Reaction Time)+Concentration at Time t

Concentration of Time of Zero Order Reaction

LaTeX Go Concentration at Time t = Initial Concentration for Zero Order Reaction-(Rate Constant of Zero Order Reaction*Reaction Time)

Rate Constant of Zero Order Reaction

LaTeX Go Rate Constant of Zero Order Reaction = (Initial Concentration for Zero Order Reaction-Concentration at Time t)/Reaction Time

Time for Completion of Zero Order Reaction

LaTeX Go Time for completion = Initial Concentration for Zero Order Reaction/Rate Constant of Zero Order Reaction

Activation Energy for Zero Order Reactions Formula

LaTeX Go

Energy of Activation = [R]*Temperature of Gas*(ln(Frequency Factor from Arrhenius Equation)-ln(Rate Constant of Zero Order Reaction))
E_a = [R]*T_gas*(ln(A)-ln(k))

What is significance of Arrhenius equation?

The Arrhenius equation explains the effect of temperature on the rate constant. There is certainly the minimum amount of energy known as threshold energy which the reactant molecule must possess before it can react to produce products. Most of the molecules of the reactants, however, have much less kinetic energy than the threshold energy at room temperature, and hence, they do not react. As the temperature is increased, the energy of the reactant molecules increases and become equal to or greater than the threshold energy, which causes the occurrence of reaction.

How to Calculate Activation Energy for Zero Order Reactions?

Activation Energy for Zero Order Reactions calculator uses Energy of Activation = [R]*Temperature of Gas*(ln(Frequency Factor from Arrhenius Equation)-ln(Rate Constant of Zero Order Reaction)) to calculate the Energy of Activation, The Activation energy for zero order reactions formula is defined as the product of universal gas constant with the temperature of the reaction and difference of natural logarithm of frequency factor and rate constant. Activation energy is the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo a chemical transformation. Energy of Activation is denoted by E_a symbol.

How to calculate Activation Energy for Zero Order Reactions using this online calculator? To use this online calculator for Activation Energy for Zero Order Reactions, enter Temperature of Gas (T_gas), Frequency Factor from Arrhenius Equation (A) & Rate Constant of Zero Order Reaction (k) and hit the calculate button. Here is how the Activation Energy for Zero Order Reactions calculation can be explained with given input values -> 30184.43 = [R]*273*(ln(149000000)-ln(250)).

FAQ

What is Activation Energy for Zero Order Reactions?

The Activation energy for zero order reactions formula is defined as the product of universal gas constant with the temperature of the reaction and difference of natural logarithm of frequency factor and rate constant. Activation energy is the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo a chemical transformation and is represented as E_a = [R]*T_gas*(ln(A)-ln(k)) or Energy of Activation = [R]*Temperature of Gas*(ln(Frequency Factor from Arrhenius Equation)-ln(Rate Constant of Zero Order Reaction)). The temperature of Gas is the measure of hotness or coldness of a gas, The Frequency Factor from Arrhenius Equation is also known as the pre-exponential factor and it describes the frequency of reaction and correct molecular orientation & The Rate Constant of Zero Order Reaction is equal to the rate of the reaction because in a zero-order reaction the rate of reaction is proportional to zero power of the concentration of the reactant.

How to calculate Activation Energy for Zero Order Reactions?

The Activation energy for zero order reactions formula is defined as the product of universal gas constant with the temperature of the reaction and difference of natural logarithm of frequency factor and rate constant. Activation energy is the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo a chemical transformation is calculated using Energy of Activation = [R]*Temperature of Gas*(ln(Frequency Factor from Arrhenius Equation)-ln(Rate Constant of Zero Order Reaction)). To calculate Activation Energy for Zero Order Reactions, you need Temperature of Gas (T_gas), Frequency Factor from Arrhenius Equation (A) & Rate Constant of Zero Order Reaction (k). With our tool, you need to enter the respective value for Temperature of Gas, Frequency Factor from Arrhenius Equation & Rate Constant of Zero Order Reaction and hit the calculate button. You can also select the units (if any) for Input(s) and the Output as well.

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