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The activation energy of the catalysed reaction is lower comparatively, which makes the effect of the temperature on rate constant much more visible when compared to the uncatalysed reaction.Īrrhenius Equation and Pre-Exponential Factor (A) This is due to the reason that the activation energy lies in the numerator of the exponential term and the absolute temperature lies in the denominator of the Arrhenius equation. You must know that the rates of the reactions that are uncatalysed are affected more severely by the temperature when compared to the rates of the catalysed reactions. As we know that the rate of the chemical reaction is proportional directly to the rate constant of that particular reaction when there is a decrease in the activation energy, the reaction rate increases exponentially.
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The exponential portion of Arrhenius equation, denoted by ( -Ea RT ) results in an exponential increase in the rate constant value when the activation energy decreases. Hence, the lowered activation energy which is accounted for the catalysts is substituted in the Arrhenius equation for getting the rate constant of the catalyzed reaction. When we plot the log of the rate constant, ln K on the Y-axis and the absolute temperature inverse ( 1 T ) on the X-axis, the graph that results is referred to as the Arrhenius plot.ĭoes Arrhenius Equation Account for the Catalysts?Ĭatalyst helps in lowering the activation energy which is needed by a particular reaction. The equation here is a straight line, y = mx + c because ln(A) is constant and has a slope denoted by m = -Ea R. When we take logarithms are on both the sides of the equation, the Arrhenius equation is written in the following manner: You must know that the reaction rate tends to increase as you increase the temperature. When the nitrogen dioxide undergoes a decomposition reaction, a graph can be plotted having the rate constant (denoted by k) plotted on the Y-axis and the absolute temperature T plotted on the X-axis.
#ARRHENIUS EQUATION CALCULATOR HOW TO#
In this article, we will learn about what is Arrhenius equation chemical kinetics, what is the Arrhenius equation derivation, and how to use the Arrhenius equation to determine the energy of activation. In case the activation energy is represented in regards to the energy per the reactant molecule, then the universal gas constant is to be replaced with another constant in the Arrhenius equation known as the Boltzmann constant, kB. T refers to the absolute temperature which is related to the reaction (denoted in Kelvin). The Arrhenius equation is given by the formula as follows:Ī refers to the pre-exponential factor which is the frequency of the properly oriented collisions between the species that are reacting.Į refers to the base of the natural logarithm, also called Euler’s number.Įa is the activation energy of the chemical reaction (denoted by energy per mole). It also provides an insight into how the reaction rates are dependent on the absolute temperature.
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The Arrhenius equation helps in providing a relationship between the rate constant of a given chemical reaction, the pre-exponential factor, A, and the absolute temperature.