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 Rate Constant for First Order Reaction from Arrhenius Equation?
Rate Constant for First Order Reaction from Arrhenius Equation calculator uses Rate Constant for First Order Reaction = Frequency Factor from Arrhenius Eqn for 1st Order*exp(-Activation Energy/([R]*Temperature for First Order Reaction)) to calculate the Rate Constant for First Order Reaction, The Rate constant for first order reaction from Arrhenius equation formula is defined as the frequency factor times the exponential of negative activation energy per universal gas constant and temperature. The rate constant of first order reaction is inversely proportional to the temperature of the reaction. As the temperature of the reaction increases the rate constant will decrease. Rate Constant for First Order Reaction is denoted by kfirst symbol.
How to calculate Rate Constant for First Order Reaction from Arrhenius Equation using this online calculator? To use this online calculator for Rate Constant for First Order Reaction from Arrhenius Equation, enter Frequency Factor from Arrhenius Eqn for 1st Order (Afactor-firstorder), Activation Energy (Ea1) & Temperature for First Order Reaction (TFirstOrder) and hit the calculate button. Here is how the Rate Constant for First Order Reaction from Arrhenius Equation calculation can be explained with given input values -> 0.520001 = 0.687535*exp(-197.3778/([R]*85.00045)).