As per the given data, a lnK vs 1/T plot is created using excel and is given in the image below:
Since slope of lnK vs 1/T plot = - Ea / R, the slope is also given in the said graph.
From the graph, Slope = -4094.9 = - Ea / R
So, Ea = 4094.9 K-1 X 8.313 J K-1mol-1 = 34040.90 J mol-1 or 34.04 kJ mol-1
first create a graph to solve the arrhenius equation for activation energy also need the graph...
Use one of your experimentally determined values of k, the activation energy you determined, and the Arrhenius equation to calculate the value of the rate constant at 25 °C. Alternatively, you can simply extrapolate the straight line plot of ln(k) vs. 1/T in your notebook to 1/298 , read off the value of ln(k), and determine the value of k. Please put your answer in scientific notation. slope=-12070, Ea=100kJ/mol, k= 0.000717(45C), 0.00284(55C), 0.00492(65C), 0.0165(75C), 0.0396(85C)
In a chemistry experiment that measures the kinetics of reaction at different temperatures, the activation energy of the reaction can be measured by finding the slope of the line in a ln k vs. 1/T plot. The following data are gathered from this kinetics experiment: ln k 1/T (K-1) -5.5886697 0.00339156 -4.8600624 0.00326318 -3.5719857 0.00313725 Construct a scatterplot of the ln k versus 1/T and fit a least-square regression line using the graph paper below. Compute the correlation coefficient between...
ause the reaction is first order wiurTo stant, k, by plotting a graph of In Absorbance vs. time. hoose New Calculated Column from the Data menu. nter "In Absorbance" as the Name, and leave the unit blank. nter the correct formula for the column into the Equation edit e Function list, and selecting "Absorbance" from the Variables list c lick on the y-axis label. Choose In Absorbance. A graph of In absorhan ow be displayed. Change the scale of the...
Need help with the first picture. Data provided in pictures #2 & #3 Determining the Activation Energy and Collision Frequency Factor for Reaction 1 Part 1. Transfer the reaction rate for runs 9.12 from Data Sheet 3. Then calculate the rate constant (R) at each temperature based on the reaction orders determined in parts and Record the results in Tables * = 18,0 ->15.0416"5,0216" Equation 6 ->25 10 2. Calculate the natural logarithm of the rate constant. In ) and...
Table 3: Experimental Data for Part 2: Determination of Activation Energy k Time* T* [1] [S,0,?] Rate (M/s) (s) (C) (M) (M) Run 3 153 20.5 .0208 .0416 4.03*10^-6 4.65*10^-3 (Room T) Run 6 198 9 .0208 .0416 3.15*10^-6 3.64*10^-3 (Cool) Run 7 112 31 .0208 .0416 5.58*10^-6 6.45*10^-3 (Warm) Run 8 40 51 .0208 .0416 1.56*10^-5 1.80*10^-2 (Warmer) 1/T (1/K) In k Run 3 1/293.5 -5.37 Run 6 1/282 -5.62 Run 7 1/304 -5.044 Run 8 1/324 -4.02 20....
just one example/demonstration! Data needed to be calculated is in highlighted in green boxes. And I highlighted in red an equation (not sure if thats what you use to calculate it) And ignore the lab instructions on completeing a graph!! I already know how to do that in excel, just curious how Ln (relative rate) and 1/T in K^-1 is calculated by hand* here is the rest of that lab leading up to the question as I know its typically...