In the process of decomposition hydrogen peroxide according to the equation:2H₂O₂-2H₂ +0₂ ; the following values data were found for the volume ofpotassium permanganate(0.02 M KMNO4) used for equivalent the hydrogen peroxideas the below:Time (min.)020406080Volume(ml.)27.3 17.010.36.33.8If you know the volume of the hydrogen peroxide 10 ml., Calculate1- The order of the reaction 2- the reaction constant mathematically 3- thereaction constant graphically1002.3

#1: In graphical determination of order, we plot three different graphs and find the order by…

In the process of decomposition hydrogen peroxide according to the equation: 2H₂O₂ potassium as the below: Time (min.) =2H₂ +0₂ ; the following values data were found for the volume of M KMNO4) used for equivalent the hydrogen peroxide permanganate(0.02 0 20 27.3 17.0 40 80 Volume(ml.) 10.3 3.8 If you know the volume of the hydrogen peroxide 10 ml., Calculate 1- The order of the reaction 2- the reaction constant mathematically 3- the reaction constant graphically 60 6.3 100 2.3

In the process of decomposition hydrogen peroxide according to the equation: 2H₂O₂ potassium as the below: Time (min.) =2H₂ +0₂ ; the following values data were found for the volume of M KMNO4) used for equivalent the hydrogen peroxide permanganate(0.02 0 20 27.3 17.0 40 80 Volume(ml.) 10.3 3.8 If you know the volume of the hydrogen peroxide 10 ml., Calculate 1- The order of the reaction 2- the reaction constant mathematically 3- the reaction constant graphically 60 6.3 100 2.3

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter13: Kinetic Methods

Section: Chapter Questions

Problem 1P

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Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
Show how equation 20.33 reduces to a simpler form of an integrated first-order rate law when the reverse reaction of an equilibrium is negligible.
The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
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The oxidation-reduction reaction between iron metal and aqueous permanganate ions in acidic solution is 16H+(aq)+5Fe(s)+2MnO4(aq)2Mn2+(aq)+5Fe2++8H2O(l) At some temperature, the reaction proceeds at such a rate that 1.00 millimole of H+ is consumed in 2 minutes 33.8 seconds. What is the invariant rate of this reaction in units of moles per second?
. Hydrogen gas and chlorine gas in the presence of light react explosively to form hydrogen chloride H2(g)+Cl2(g)2HCl(g)The reaction is strongly exothermic. Would an increase in temperature for the system lend to favor or disfavor the production of hydrogen chloride?
11.41 For a drug to be effective in treating an illness, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30 min. If a person receives an injection of 25 mg of penicillin at t = 0, how much penicillin remains in the body after 3 hours?
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
The gas-phase reaction between hydrogen and iodine H2(g)+I22HI(g)proceeds with a rate constant for the forward reaction at 700C of 138 L/moI s and an activation energy of 165 kJ/moI. (a) Calculate the activation energy of the reverse reaction given that H f for HI is 26.48 kJ/moI and H f for I2(g) is 62.44 kJ/mol. (b) Calculate the rate constant for the reverse reaction at 700C. (Assume A in the equation k=AeE a /RT is the same for both forward and reverse reactions.) (c) Calculate the rate of the reverse reaction if the concentration of HI is 0.200 M. The reverse reaction is second-order in HI.
Assume that thermal decomposition of mercuric oxide, HgO, follows first-order kinetics. It can be followed by the production of oxygen gas as a product: 2HgO(s)2Hg(l)+O2(g) At a particular temperature, k=6.02104s1. If 1.00gram of HgO were present initially, how long would it take to produce a1.00mL of O2(g) at STP; b10.0mL of O2(g) at STP? STP = standard temperature and pressure for a gas.