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Test your understanding in this question below: Chemistry by OpenStax is licensed under Creative Commons Attribution License v4.0. where temperature is the independent variable and the rate constant is the dependent variable. However, because \(A\) multiplies the exponential term, its value clearly contributes to the value of the rate constant and thus of the rate. A is known as the frequency factor, having units of L mol-1 s-1, and takes into account the frequency of reactions and likelihood of correct molecular orientation. Arrhenius Equation Calculator - calctool.org What is "decaying" here is not the concentration of a reactant as a function of time, but the magnitude of the rate constant as a function of the exponent Ea/RT. 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. $$=\frac{(14.860)(3.231)}{(1.8010^{3}\;K^{1})(1.2810^{3}\;K^{1})}$$$$=\frac{11.629}{0.5210^{3}\;K^{1}}=2.210^4\;K$$, $$E_a=slopeR=(2.210^4\;K8.314\;J\;mol^{1}\;K^{1})$$, $$1.810^5\;J\;mol^{1}\quad or\quad 180\;kJ\;mol^{1}$$. The Arrhenius equation allows us to calculate activation energies if the rate constant is known, or vice versa. Determining the Activation Energy . Math Workbook. An open-access textbook for first-year chemistry courses. Arrhenius Plots - Video - JoVE Equation \ref{3} is in the form of \(y = mx + b\) - the equation of a straight line. A is called the frequency factor. You can also change the range of 1/T1/T1/T, and the steps between points in the Advanced mode. Two shaded areas under the curve represent the numbers of molecules possessing adequate energy (RT) to overcome the activation barriers (Ea). This approach yields the same result as the more rigorous graphical approach used above, as expected. Our answer needs to be in kJ/mol, so that's approximately 159 kJ/mol. When you do, you will get: ln(k) = -Ea/RT + ln(A). So k is the rate constant, the one we talk about in our rate laws. Activation Energy and the Arrhenius Equation - Lumen Learning