please help me with question-23, how to calculate rate constant. I am unsure about the values of m and n of k[S2O8^2-]m [I-]n

All the required data is posted here including equations.

thank you for your help : )

Construct a plot of In [relative rate 100] vs. 1/T. For [relative rate x 100], multiply each relative rate by 100 . This procedure gives you more manageable numbers to graph, but it in no way affects the slope: it simply moves the graph up the page. Add a line of best fit based on the five data points. Note, this line probably won't go through any of the data points. Find the slope. From the slope calculate E3. Review "Graphs in First-Year Chemistry" in the introduction to the lab manual. Part 1 - Dependence of Reaction Rate on Concentration The activation energy may be thought of as the height of the energy barrier over which the reactants must pass in going to products. A catalyst increases the rate of a reaction without itself being consumed. It does so by providing a new reaction pathway with a lower activation energy, and thus a larger rate constant. The Reaction In this experiment, we will study the rate of the reaction of peroxydisulfate ion, S2O22, with iodide ion, I, in aquecus solution. The reaction is described by the following equation: S2O2(aq)+3H(aq)l(aq)+2SO2(aq) The reaction is described as homogeneous because all reactants are in the same phase. In this case, the phase is aqueous solution. Our first problem is to determine how the rate of this reaction depends upon the concentrations of S2O82 and 1-. If we choose to study the rate by determining the rate of consumption of peroxydisulfate ion, that is, the change of S2O82-concentrationwith. time, then the problem is stated mathematically by the equation: dtd[S2O12]=k[S2On2]4[I] where we must determine the values of m and n by experiment. To determine m we must study the effect of changing the concentration of S2O32 while keeping the concentration of Fconstant. This can be accomplished by making use of thiosulfate ion, S2O2, which reacts with Ias soon as it is formed, to regenerate 1 . I(aq)+2S2O22(aq)3T(aq)+SiO32(aq) Because this reaction is much more rapid than the reaction of S2O32 with I(Equation 6), the I ion concentration remains constant as long as some S2O32 is present. We will add a small quantity (5.00105mol) of the thiosulfate ion, S2O22, to the solution of S2O52 under study. As the S2O82 and t react, is will be formed but this I3- will immediately react with S2Oy2 (Equation B) to form S4Oo2 and to regenerate IOnly when all of the 5.00105 mole of thiosulfate is consumed will any detectable amount of l3 exist in the solution. We can detect the presence of Iby adding sorme starch to the solution. Starch forms an intense blue-black colour with ls-. Thereforo. the appearance of the blue colour signals that all of the S2Oy2 - has been consumed. Because each mole of S2O2 consumed produces one mole of 5(Equation 6), and Remember: Although data acquisition is performed with a partner, all analysis (e.g. calculations, graphs, etc.) must be performed independently. Part 1 - Dependence of Reaction Rate on Concentration 1. Experimental set-up: a) In Part 1, you will prepare five different reactions. For each reaction, you will need a 250mL and 50mL beaker. The beakers must be clean, but they may be wet. b) Refer to Table 1 below, which details the solutions provided and the corresponding glassware to use for their measurement. c) Table 2 (on the following page) indicates which solutions are required for each reaction and dictates which solutions should be prepared in which beaker. d) Carefully label each beaker, and any other containers, using a small piece of masking tape. e) Ensure that you are using the correct solution(s). Read labols twice before obtaining chemicals. Although there are similarly named reagents, they are not interchangeable. Table 1. Solutions provided and glassware to use. EXP. 4 CHEMICAL KINETICS Table 2. Solutions for each reaction TEDTA (othylenediaminetotrascetic acid) is added to form a complex with any traces of transition metal cation impurites which may act as catalysts. TKNO; and (NH)LSO, soluticns are used rather than water for dilutions to keep the ianic strength of each solution, which affocts the reoction rate, essentialy the same. 2. Prepare the solutions for Reaction 1: a) Measure the (NH4)2S2O3 solution from the burette into a clean, wet 50 mL beaker. This beaker must be very, very clean. Scrub it and rinse with deionized water. It should drain without leaving drops clinging to the surface. b) Fasten your thermometer, or hold it by hand, such that the bulb dips into the lodide solution in the reaction beaker (250mL). c) Note: The reaction begins when (NH4)2S2O is added to the KI solution mixture. Therefore, all must be ready prior to adding the 50mL beaker contents to the 250mL beaker. Be prepared to start timing the reaction immediately upon mixing the solutions. To ensure the last drop of (NH2)2S2O is is added to the reaction vessel either touch the lip of the 50mL beaker to the wall of the 250mL beaker or let the drops of (NH4)2S2O2 flow down a glass rod held in contact with the lip. Question 23 (3 points) Using your own lab-obtained data, calculate the rate constant, k, for Part 1 Reaction \#5. State any previously calculated values you are using, but only show the calculation for the rate constant. Explain any assumptions you make. Construct a plot of In [relative rate 100] vs. 1/T. For [relative rate x 100], multiply each relative rate by 100 . This procedure gives you more manageable numbers to graph, but it in no way affects the slope: it simply moves the graph up the page. Add a line of best fit based on the five data points. Note, this line probably won't go through any of the data points. Find the slope. From the slope calculate E3. Review "Graphs in First-Year Chemistry" in the introduction to the lab manual. Part 1 - Dependence of Reaction Rate on Concentration The activation energy may be thought of as the height of the energy barrier over which the reactants must pass in going to products. A catalyst increases the rate of a reaction without itself being consumed. It does so by providing a new reaction pathway with a lower activation energy, and thus a larger rate constant. The Reaction In this experiment, we will study the rate of the reaction of peroxydisulfate ion, S2O22, with iodide ion, I, in aquecus solution. The reaction is described by the following equation: S2O2(aq)+3H(aq)l(aq)+2SO2(aq) The reaction is described as homogeneous because all reactants are in the same phase. In this case, the phase is aqueous solution. Our first problem is to determine how the rate of this reaction depends upon the concentrations of S2O82 and 1-. If we choose to study the rate by determining the rate of consumption of peroxydisulfate ion, that is, the change of S2O82-concentrationwith. time, then the problem is stated mathematically by the equation: dtd[S2O12]=k[S2On2]4[I] where we must determine the values of m and n by experiment. To determine m we must study the effect of changing the concentration of S2O32 while keeping the concentration of Fconstant. This can be accomplished by making use of thiosulfate ion, S2O2, which reacts with Ias soon as it is formed, to regenerate 1 . I(aq)+2S2O22(aq)3T(aq)+SiO32(aq) Because this reaction is much more rapid than the reaction of S2O32 with I(Equation 6), the I ion concentration remains constant as long as some S2O32 is present. We will add a small quantity (5.00105mol) of the thiosulfate ion, S2O22, to the solution of S2O52 under study. As the S2O82 and t react, is will be formed but this I3- will immediately react with S2Oy2 (Equation B) to form S4Oo2 and to regenerate IOnly when all of the 5.00105 mole of thiosulfate is consumed will any detectable amount of l3 exist in the solution. We can detect the presence of Iby adding sorme starch to the solution. Starch forms an intense blue-black colour with ls-. Thereforo. the appearance of the blue colour signals that all of the S2Oy2 - has been consumed. Because each mole of S2O2 consumed produces one mole of 5(Equation 6), and Remember: Although data acquisition is performed with a partner, all analysis (e.g. calculations, graphs, etc.) must be performed independently. Part 1 - Dependence of Reaction Rate on Concentration 1. Experimental set-up: a) In Part 1, you will prepare five different reactions. For each reaction, you will need a 250mL and 50mL beaker. The beakers must be clean, but they may be wet. b) Refer to Table 1 below, which details the solutions provided and the corresponding glassware to use for their measurement. c) Table 2 (on the following page) indicates which solutions are required for each reaction and dictates which solutions should be prepared in which beaker. d) Carefully label each beaker, and any other containers, using a small piece of masking tape. e) Ensure that you are using the correct solution(s). Read labols twice before obtaining chemicals. Although there are similarly named reagents, they are not interchangeable. Table 1. Solutions provided and glassware to use. EXP. 4 CHEMICAL KINETICS Table 2. Solutions for each reaction TEDTA (othylenediaminetotrascetic acid) is added to form a complex with any traces of transition metal cation impurites which may act as catalysts. TKNO; and (NH)LSO, soluticns are used rather than water for dilutions to keep the ianic strength of each solution, which affocts the reoction rate, essentialy the same. 2. Prepare the solutions for Reaction 1: a) Measure the (NH4)2S2O3 solution from the burette into a clean, wet 50 mL beaker. This beaker must be very, very clean. Scrub it and rinse with deionized water. It should drain without leaving drops clinging to the surface. b) Fasten your thermometer, or hold it by hand, such that the bulb dips into the lodide solution in the reaction beaker (250mL). c) Note: The reaction begins when (NH4)2S2O is added to the KI solution mixture. Therefore, all must be ready prior to adding the 50mL beaker contents to the 250mL beaker. Be prepared to start timing the reaction immediately upon mixing the solutions. To ensure the last drop of (NH2)2S2O is is added to the reaction vessel either touch the lip of the 50mL beaker to the wall of the 250mL beaker or let the drops of (NH4)2S2O2 flow down a glass rod held in contact with the lip. Question 23 (3 points) Using your own lab-obtained data, calculate the rate constant, k, for Part 1 Reaction \#5. State any previously calculated values you are using, but only show the calculation for the rate constant. Explain any assumptions you make