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The Arrhenius EquationBackground reading:Common sense and chemical intuition suggest that the higher the temperature, the faster a given chemical reaction will proceed. Quantitatively this relationship between the rate a reaction proceeds and its temperature is determined by the Arrhenius Equation. At higher temperatures, the probability that two molecules will collide is higher. This higher collision rate results in a higher kinetic energy, which has an effect on the activation energy of the reaction. The activation energy is the amount of energy required to ensure that a reaction happens.This calculator calculates the effect of temperature on reaction rates using the Arrhenius equation.
R has the value of 8.314 x 10^{3} kJ mol^{1}K^{1} You should use this calculator to investigate the influence of temperature on the rate coefficient. This calculator allows you to perform three different calculations:
Sample Problem:The reaction:
has a rate coefficient of 1.0 x 10^{10} s^{1} at 300 K and an activation energy of 111 kJ mol^{1}. What is the rate coefficient at 273 K? (Solution: calculate the value of A for a temperature of 300 K, then use the calculated value of A to calculate k at a temperature of 273 K. We generally assume that A and the activation energy E_{a }do not vary with temperature).
Calculate k given A, E_{a}, and T:Calculate E_{a} given A, k, and T:Back to the kinetics page. 
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