1. The rate of reaction depends upon (a) the concentration and nature of the reactants (b) the temperature of the reaction (c) whether or not a catalyst was used (d) all of the above 2. What are the units of the rate constant, k, in a secondorder equation if rate is measured in mol/ (L . s) and all concentrations are in mol/L? (a) (b) L/(mol·s) (c) L²/(mol²-s) (d) mol?/(L²-s) 3. Which of the following statements is true, according to the collision theory? (a) All collisions result in reactions. (b) Entities must collide to react. (c) Entities that collide but are incorrectly oriented will form a different product. (d) All entities in a collision have the same quantity of kinetic energy. 4. Which of the following properties is NOT required to determine the amount of thermalenerg needed to raise the temperature of a substance? (a) mass (b) volume (c) temperature change (d) specific heat capacity

1. The rate of reaction depends upon (a) the concentration and nature of the reactants (b) the temperature of the reaction (c) whether or not a catalyst was used (d) all of the above 2. What are the units of the rate constant, k, in a secondorder equation if rate is measured in mol/ (L . s) and all concentrations are in mol/L? (a) (b) L/(mol·s) (c) L²/(mol²-s) (d) mol?/(L²-s) 3. Which of the following statements is true, according to the collision theory? (a) All collisions result in reactions. (b) Entities must collide to react. (c) Entities that collide but are incorrectly oriented will form a different product. (d) All entities in a collision have the same quantity of kinetic energy. 4. Which of the following properties is NOT required to determine the amount of thermalenerg needed to raise the temperature of a substance? (a) mass (b) volume (c) temperature change (d) specific heat capacity

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 11.100PAE

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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?
Diethylhydrazine reacts with iodine according to the following equation: Â (C2H5)2(NH)2(l)+I2(aq)(C2H5)2N2+2HI(aq)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) What is the order of the reaction with respect to diethylhydrazine, iodine, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) What must [(C2H5)2] be so that the rate of the reaction is 5.00104mol/Lh when [ I2 ]=0.500M?
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?
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For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.
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Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]