1-arrIn a study of the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °CN2O5-→2 NO2 + ½ O2the concentration of N,O5 was followed as a function of time.It was found that a graph of In[N2O5] versus time in minutes gave a straight line with a slope of -6.31×10* min and a y-intercept of -1.34 .Based on this plot, the reactionO order in N,0g and the rate constant for the reaction ismin-1.zerofirstsecond

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1-arr In a study of the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N,O5 →2 NO2 + ½ O2 the concentration of N,O5 was followed as a function of time. It was found that a graph of In[N,O5] versus time in minutes gave a straight line with a slope of -6.31×103 min1 and a y- intercept of -1.34 . Based on this plot, the reactioni v O order in N,Og and the rate constant for the reaction is min-1. zero first second

1-arr In a study of the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N,O5 →2 NO2 + ½ O2 the concentration of N,O5 was followed as a function of time. It was found that a graph of In[N,O5] versus time in minutes gave a straight line with a slope of -6.31×103 min1 and a y- intercept of -1.34 . Based on this plot, the reactioni v O order in N,Og and the rate constant for the reaction is min-1. zero first second

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter13: Kinetic Methods

Section: Chapter Questions

Problem 3P

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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 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.
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Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
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Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?