Need a lab report Write paragraphs in Abstract, introduction, Safety . And follow the experiment MEMO and the experiment procedure to know what data you should calculate.

Problem 4. Activation energy Razavi, Blagodatskaya, and Kuzyakox (2015) found the maximum rate of xylanase in soil samples at different temperatures. They used a sample size of 0.5 g of soil and an enzyme concentration of 1 umol, the results are in the following table: a) Calculate the values of KCAT and the energy of activation of the reaction.

You will need the following data:R = 8.314 kPa L molK1I from the information above in KelvinV from the information above in LP in kPaNote: the units all have to be in the same form when used in calculations!!!100% H2O2 density is 1.45 g/mL5 mL of a solution containing an unknown concentration of hydrogen peroxide wasdecomposed at 25 °C releasing 48 mL of gas. The temperature of the container used to measure the volume of gas produced was 20 °C.To find BOTH the concentration of hydrogen peroxide in the solution AND the percentage of hydrogen peroxide in solution work through the following steps.1.Rearrange the ideal gas law to solve for n.2. Convert the temperature of the water in the collection vessel from °C to Kelvin (K). Therefore: T =3.Convert the current barometric pressure in the room from hPa to kPa. The Macquarie university weather station data can be used to find the pressure http://aws.mq.edu.au.Use the current pressure which is given in hectopascals. Use 1018 hPa if unavailable.10 hPa = 1 kPa So divide hPa by 10 to convert to kPa.Convert the volume of oxygen from mL to Liters and solve for the number of moles ofO2. Be sure the units cancel so that you end up with only the moles of O2.

12. Plot the data above (volume vs time in sec) on graph paper and draw the line-of-best-fit through the first 3 or 4 of the data points.(Graph paper given. Label axes correctly)13. From the slope (rise over run) of this line of best fit what is the initial rate of reaction in mL O2 produced per sec.14. Convert this to mol/sec using the ideal gas law.15. Convert this to rate of reaction of hydrogen peroxide reacted per sec. (Hint: This will be twice the rate of oxygen production based on the stoichiometry as two H2O2 decompose to make one O2.) 16. Convert this to concentration of hydrogen peroxide reacted per second in the reaction(Assume the reaction volume is 10 mL and the units are mol L's').