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Arrhenius Equation Lab Report

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The graph for the lab of ln k versus 1/T displays a line of best fit with a negative slope and an R^2 value of 0.9544, showing that the line fits reasonably well with the data provided. This negative trend shows that as 1/T increases, the value of the natural log of the reaction constant will decrease. This linear trend and the equation that was created for it of y=-4687.6x + 24.181 is what is expected due to its relationship with the Arrhenius equation ln⁡k=-E_a/R (1/T)+ln⁡A. The Arrhenius equation in this form is meant to resemble the format of the linear equation y = mx + b. The Arrhenius equation closely resembles the equation that was obtained for the slope of the line for the graph. By using this comparison, the activation energy of the …show more content…

The temperature of the solutions were changed in order to measure the time of the reaction. This time was then used in order to calculate the reaction rate using equation 2. By looking at the relationship between temperature and time of a reaction, it can be seen that as the temperature of a solution increases the time for a reaction decreases. This leads to the reaction rate increasing as the temperature increases. The calculated reaction rates for the trials were then used in order to calculate the reaction constant using equation 4. These reaction constants show that as the temperature of a reaction changes then the reaction constant will change as well. These values for reaction constants along with the values for temperature in Kelvin were used in order to create Graph 1 of ln k versus 1/T. The equation y = -4687.6x + 24.181 was obtained from the graph as a line of best fit and was compared to the Arrhenius equation ln⁡k=-E_a/R (1/T)+ln⁡A. The similarities between the two equation allows us to calculate the activated energy of 38.97 kJ/mol using equation 6. Due to this the purpose of the lab was

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