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1. The rate law for the reaction between catalase and hydrogen peroxide can be written as Rate = k [H2O2] x [catalase]y . A catalase solution of unknown, but constant concentration is prepared. Can the partial order with respect to the peroxide (x) be found using this catalase solution? If so, how would you do it? Describe in detail the steps you would take or show a calculation.
2. At 20.0oC, a student studying the catalase-catalyzed decomposition of hydrogen peroxide obtained an initial rate of formation of oxygen of 0.46 mL s -1 . At 30.0 and 37.0oC, the student obtained initial rates of 0.63 and 0.73 mL s -1 . What was the value of the activation energy that the student obtained?
3. A student obtained the following data for the iodide-catalyzed decomposition of hydrogen peroxide in a trial at 30.0oC: Time (s) Pressure O2 formed (kPa) 0.20 103.63 0.40 104.19 0.60 104.75 0.80 105.30 1.00 105.86 What initial rate was the student able to calculate for the iodide-catalyzed decomposition of hydrogen peroxide at 30.0oC?
4. For an experimental study of the kinetics of hydrogen peroxide decomposition in which the pressure of oxygen or volume of oxygen is monitored as a function of time, what should the volume of oxygen collected or the pressure of oxygen be at time zero? Do you expect your plot to pass through the origin? If so, why? If not, why not?
The first ionization energy for rubidium is +403.0KJ/mol. How much energy would be required to convert 17.1g of gaseous rubidium to its gaseous +1 monatomic ion at constant temperature
Given the following balanced chemical equation, calculate the mass of each reactant and each product, and then answer the questions below.
Vinegar, which is just a dilute acetic acid solution, is very common and versatile. The concentration of store-bought vinegar around a 5.0 % solution by mass, and its density is approximately 1.01 g/mL. (a) Suppose I dilute this vinegar into a bottle..
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Once this is done, the moles can be converted to grams by using the molecular weight of KHP (HC8H4O4K). Show method of calculations.
How efficient is the extraction of tea leaves containing 1.0 g of caffeine with two 30-mL portions of chloroform over that of a single step extraction (K25ºC = 8.36)?
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