A researcher was analyzing a data set from an initial rate experiment for the reactionof baking soda and vinegar at 25°C.NaHCO3 + HC2H3O2CO2 + H20 + NaC2H3O2Experiment [NaHCOgl. M[HC2H3O2), Mrate (M/s)3.0001.5000.7500.4000.4000.03600.018030.4000.0090The researcher suggested the following rate law based on these results: rate =k[NaHCO), with a k 0.012 s. Do you agree with the researchers conclusion, whyor why not. O CHEM1212

Answered: Image /qna-images/answer/f02465d1-e9b3-4b7c-9706-ecc06ecf6419.jpg

A researcher was analyzing a data set from an initial rate experiment for the reaction of baking soda and vinegar at 25°C. NaHCO3 + HC2H02 CO2 + H2O+ NaC2H3O2 Experiment [NaHCO3]. M[HC2H302). Mrate (M/s) 1 3.000 0.0360 0.0180 0.0090 0.400 1.500 0.400 3 0.750 0.400 The researcher suggested the following rate law based on these results: rate = k[NaHCO3], with a k 0.012 s. Do you agree with the researchers conclusion, why or why not. © CHEM1212

A researcher was analyzing a data set from an initial rate experiment for the reaction of baking soda and vinegar at 25°C. NaHCO3 + HC2H02 CO2 + H2O+ NaC2H3O2 Experiment [NaHCO3]. M[HC2H302). Mrate (M/s) 1 3.000 0.0360 0.0180 0.0090 0.400 1.500 0.400 3 0.750 0.400 The researcher suggested the following rate law based on these results: rate = k[NaHCO3], with a k 0.012 s. Do you agree with the researchers conclusion, why or why not. © CHEM1212

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 17E: Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft...

See similar textbooks

Similar questions

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.
11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
What is the difference between average rate, initial rate, and instantaneous rate?
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5 C. (a) Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. (b) Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other?
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?
6. Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5°C. Time (s) [Phenyl acetate] (mol/L) 0 0.55 15.0 0.42 30.0 0.31 45.0 0.23 60.0 0.17 75.0 0.12 90.0 0.085 Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other? What is the rate of change of the phenyl acetate concentration during the time period 60.0 seconds to 75.0 seconds? What is the instantaneous rate at 15.0 seconds?