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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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The reaction was repeated 3 times and average rate noted. From these rates a graph was plotted which describes the relationship of the pressure produced and number of drops added. The reaction rates were measured by Kpa/min and were written to 4 figures for precise results. Time was measured by stop watch. Table 4 shows a summary of all the groups which participated in the lab session.

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289 Words | 2 Pages

We found that Joules from NaCl = 340 J, NH4NO3 = 1340 J, CaCl2 = -2320 J, LiCl = -3600, Na2Cl3 = -720 J, NaC2H3O2= 1070 J. Then we used energy release from one one these rxn to calculate the Hor the KJ per mol rxn.

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79 Words | 1 Pages

How is temperature related to this reaction? The higher the temperature the slower they move.

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Table 1 Results DDA Concentration Initial Mass(g) Time Interval Recovered Mass Cumulative Mass (g) Cumulative Recovery (%) Ln[(Rinf -R)/ Rinf] R=Rinf(1-e-kt) (M) (g) 10^(-5) 160 0 0

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Using this number as well as the theoretical yield, the percentage yield was calculated and can be seen below in Figure 5. % Yield: (0.1805 g)/(0.3064 g) x 100 = 58.92% Figure 5: The calculations of the percent yield. The percentage yield was calculated to be 58.92% and this represents that a portion of the reactants were lost during the experiment due to a small spill or improper collection of the product during the purification process. Next, the spectrum of the product was obtained.

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1528 Words | 7 Pages

For example, in 20% catalase concentration, the reaction rate was 2.48 mm/s; then in 40% catalase concentration, the reaction rate was 2.75 mm/s; lastly in 100% catalase concentration, the rate of reaction was .84 mm/s. The reason why the increase of catalase concentration would lead to the increase of the reaction rate was due to the Collision Theory. Collision theory is a theory used to predict the rate of chemical reaction, especially for gases. The theory is based on the assumption that for one reaction to occur, it is necessary to have reactant collide with one another. A collision that could produce chemical change would be effective only if the reaction brought together possess a certain amount of internal energy, which is equal to the activation energy of the reaction. Nonetheless, the colliding reactions must be oriented to suit the necessary rearrangement of atoms and electrons.

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This activity answered the question of how to find the amounts of products and reactants within a chemical reaction. The amount of reactant produced by a chemical equation can be found by finding the limiting reactant. In order to find the limiting reactant, one must use stoichiometry to find which product produces the least amount of the reactant. The lowest answer is the limiting reactant. This activity had many models to help explain what the limiting reactant is and how it can be found.

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This occurs due to the fact that as temperature increases the kinetic energy, and thus the speed of the particles, increases. Subsequently, as the kinetic energy in the particles increase, the number of times the particles make contact, and have sufficient speed, grow allowing the rate of the reaction to increase. As a result, three different temperatures have been tested, one at room temperature, one at approximately 71oC, and another at roughly -4oC.

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To determine the rate of reaction there are many method to be used for example, measuring the mass after the product has been added and measuring the difference in mass on the duration of a digital scale. Another method, which will be used in this experiment is using a gas syringe to measure the volume of the gas which has been produced. The cylinder inside, will be pushed out to show a quantitative presentation of the volume produced by the reaction. Hypothesis

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Since temperature if a factor that affects the rate of the reaction, it could have slowed it down. Part 2 demonstrated how an increase in temperature also speeds up the reaction. This is due to the fact that the increase in temperature increases the average kinetic energy of the reactant molecules, which in turn increases the collision frequency. The increase in temperature sped the rate of the reaction from 0.0363 mL/s at 23oC to 0.062 mL/s at 37oC, meaning the rate of the reaction almost doubled with an increase in

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1524 Words | 7 Pages

The gradient gave the value of K, the rate constant for the reaction. Figure 2 shows the plotted graph Figure 2. From the

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Predict/ roughly determine the Vmax and ½ Vmax values from the peak of the graph, where the slope of the graph levels off (the asymptotical line). Predict/ roughly determine the Km by reading off of the graph the corresponding substrate concentration on the x-axis for the ½ Vmax value. Plot a Lineweaver-Burke graph (the inverse of the velocity of the reaction vs. the inverse of the substrate concentration). Calculate accurate Vmax and Km values using the following equation for the Lineweaver-Burk

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Lab Report Experiment 6 Rates of Chemical Reactions By Nikhola Mirashirova Lab Partner: Dina Abetova Section 3, Saturday October 31, 2015 Introduction Rate reaction is the measure of the change in concentration of the reactants or the change in concentration of the products per unit time.1,2 Rate law for this experiment: Rate = k(I-)m(BrO3-)n(H+)p There are several factors which affect the rate of reaction: catalyst, reactant concentration, and temperature.1,2 A catalyst is a substance that changes, increases or decreases, the rate of a chemical reaction but is not being used up during the reaction.3 It provides an alternative way, so that the rate of reaction changes.4 Catalyst, which is used in this experiment, is (NH4)2MoO (0.5 M).

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1054 Words | 5 Pages

℃^(-1)×6.40℃±3.1 %=1337.6 J±4.06 % ∆H=(-1337.6 J±4.06 %) /(0.025 mol ±0.16 %)= -53504 J m〖ol〗^(-1)±4.22 % ∆H=-53504 J m〖ol〗^(-1)±4.22 %÷1000=-54 kJ m〖ol〗^(-1)±4.22 % Conclusion and

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3578 Words | 15 Pages

When R2 equals 1.0, all points lie exactly on a straight line with no scatter. Knowing X lets you predict Y perfectly. (http://www.graphpad.com/guides/prism/6/curve-fitting/index.htm?r2_ameasureofgoodness_of_fitoflinearregression.htm) In this graph the R2 value is 0.97 which can be rounded off to 1.0 which means that knowing X which in this case is the different concentrations of sodium thiosulfate, predicts the Y which is the time the time the solution turns cloudy resulting X not to be seen from the opening of the conical flask from a person’s eye

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