Darlana Finding half life and rate constant from a graph of concentratio... A chemical engineer is studying the rate of this reaction 2NH3 g)N2 (g)+3H2 (g) He fills a reaction vessel with NH2 and measures its concentration as the reaction proceeds. Here's a graph of his data: dlo (seconds) ()[HN lII U KINETICS AND EQUILIBRIUM Dariana Finding half life and rate constant from a graph of concentratio... Use this graph to answer the following questions: What is the half life of the reaction? to Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in NH2. Calculate the value of the rate constant k. X k = Round your answer to 2 significant digits. Also be sure you include the correct unit symbol Ar Predict the concentration of NH2 in the engineer's reaction vessel after 6.0 seconds have passed NH, M Assume no other reaction is important, and continue to assume the rate is first order in NH3. Round your answer to 2 significant digits.

Darlana Finding half life and rate constant from a graph of concentratio... A chemical engineer is studying the rate of this reaction 2NH3 g)N2 (g)+3H2 (g) He fills a reaction vessel with NH2 and measures its concentration as the reaction proceeds. Here's a graph of his data: dlo (seconds) ()[HN lII U KINETICS AND EQUILIBRIUM Dariana Finding half life and rate constant from a graph of concentratio... Use this graph to answer the following questions: What is the half life of the reaction? to Round your answer to 2 significant digits. Suppose the rate of the reaction is known to be first order in NH2. Calculate the value of the rate constant k. X k = Round your answer to 2 significant digits. Also be sure you include the correct unit symbol Ar Predict the concentration of NH2 in the engineer's reaction vessel after 6.0 seconds have passed NH, M Assume no other reaction is important, and continue to assume the rate is first order in NH3. Round your answer to 2 significant digits.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.48PAE: 11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol...

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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.
What is the difference between average rate, initial rate, and instantaneous rate?
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When nitrogen dioxide reacts with carbon monoxide, the following reaction occurs. Â NO2(g)+CO(g)NO(g)+CO2(g)The following data are obtained at a certain temperature: (a) What is the order of the reaction with respect to NO2, CO, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) When [ NO2 ]=0.421Mand [ CO ]=0.816M, what is the rate of the reaction at the temperature of the experiments?
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.
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At low temperatures, the rate law for the reaction CO(g)+NO2(g)CO2(g)+NO(g)is as follows: rate=(constant)[ NO2 ]2. Which of the following mechanisms is consistent with the rate law? (a) CO+NO2CO2+NO(b) 2NO2N2O4(fast) N2O4+2CO2CO2+2NO(slow) (c) 2NO2NO3+NO(slow) NO3+CONO2+CO2(fast) (d) 2NO22NO+O2(slow) O2+2CO2CO2(fast)
Consider the first-order decomposition of phosgene at a certain temperature. COCl2(g)productsIt is found that the concentration of phosgene is 0.0450 M after 300 seconds and 0.0200 M after 500 seconds. Calculate the following: (a) the rate constant at the temperature of the decomposition (b) the half-life of the decomposition (c) the intial concentration of phosgene
Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]
Nitric oxide, NO, is known to break down ozone, O3, by the following bimolecular reaction: NO(g)+O3(g)NO2(g)+O2(g) If the activation energy of this reaction is 10.5kJ/mol and the pre-exponential factor is 7.91011cm3/(mols), a what is the rate constant of this reaction at 298K? b If the ozone concentration were 5.41012mol/cm3 and the NO concentration were 2.01012mol/cm3 conditions that might exist in a high-pollution area, what is the rate of this reaction?
Consider the following hypothetical reaction: X( g )Y( g ) A 200.0-mL flask is filled with 0.120 moles of X. The disappearance of X is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the appearance of Y. (b) Calculate the average disappearance of X in M/S in the first two 20-minute intervals. (c) What is the average rate of appearance of Y between the 20- and 60-minute intervals?
The nitration of methanol, CH3OH, by nitrous acid is thought to proceed via the following mechanism: CH3OH+H+CH3OH2+CH3OH2+CH3++H2OCH3++NO2CH3NO2 Suppose the first step is the RDS. What is the expected rate law in terms of the original reactants?