In a study of the gas phase decomposition of sulfuryl chloride at 600 Kso,Ch(gSO;(g) + Cl,(g)the concentration of SO,Clh was followed as a function of time.It was found that a graph of In[SO,Cl] versus time in minutes gave a straight line with a slope of -3.92x103 min and a y-intercept of -5.69.Based on this plot, the reaction isorder in SO,Cl, and the rate constant for the reaction i |min-!Submit AnswerRetry Entire Group8 more group attempts remaining The decomposition of nitramide in aqueous solution at 25 °CNH,NO,(ag) → N,0(g) + H,O(1)is first order in NH,NO, with a rate constant of 4.70×10-5 5-1.If the initial concentration of NH,NO, is 0.202 M, the concentration of NH,NO, will be]Mafter 38207 s have passed.Submit AnswerRetry Entire Group8 more group attempts remaining

There are various kinds of rate of reaction on basis of the dependance to the reactant…

In a study of the gas phase decomposition of sulfuryl chloride at 600 K SO̟Cl,(g)SO,(g) + Cl½(g) the concentration of So,Cl, was followed as a function of time. It was found that a graph of In[SO,Cl,] versus time in minutes gave a straight line with a slope of -3.92×103 minl and a y-intercept of -5.69 . Based on this plot, the reaction is | order in SO,Cl, and the rate constant for the reaction is min-!.

In a study of the gas phase decomposition of sulfuryl chloride at 600 K SO̟Cl,(g)SO,(g) + Cl½(g) the concentration of So,Cl, was followed as a function of time. It was found that a graph of In[SO,Cl,] versus time in minutes gave a straight line with a slope of -3.92×103 minl and a y-intercept of -5.69 . Based on this plot, the reaction is | order in SO,Cl, and the rate constant for the reaction is min-!.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.3CE

See similar textbooks

Similar questions

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.
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
The isomerization reaction CH3NCCH3CN obeys the first-order rate law rate=k[CH3NC] in the presence of an excess of argon. Measurementsat500 K reveal that in 520 s theconcentration of CH3NC decreases to 71% of its original value. Calculate the rateconstant k of the reaction at 500 K.
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.
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
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?
List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
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.
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.