A chemical engineer is studying the rate of this reaction. NH,OH (aq) → NH, (aq)+H,O (aq) He fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.20 (W) [HO'HN] 0.15- 0.10. 0.05. 0.2 0.4 0.6 (5) Use this graph to answer the following questions: What is the half life of the reaction? Round your answer to 2 significant digits. Suppose the rate of the reaction 72-08 S known to be first order in k = -0 NH4OH. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of NH4OH in the engineer's reaction vessel after 1.20 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in NH4OH. Round your answer to 2 significant digits. [NH₂OH]-M 0.0 X G ים

A chemical engineer is studying the rate of this reaction. NH,OH (aq) → NH, (aq)+H,O (aq) He fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.20 (W) [HO'HN] 0.15- 0.10. 0.05. 0.2 0.4 0.6 (5) Use this graph to answer the following questions: What is the half life of the reaction? Round your answer to 2 significant digits. Suppose the rate of the reaction 72-08 S known to be first order in k = -0 NH4OH. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure you include the correct unit symbol. Predict the concentration of NH4OH in the engineer's reaction vessel after 1.20 seconds have passed. Assume no other reaction is important, and continue to assume the rate is first order in NH4OH. Round your answer to 2 significant digits. [NH₂OH]-M 0.0 X G ים

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 11.99PAE: Substances that poison a catalyst pose a major concern for many engineering designs, including those...

See similar textbooks

Similar questions

. Account for the increase in reaction rate brought about by a catalyst.
How do chemists envision reactions taking place in terms of the collision model for reactions? Give an example of a simple reaction and how you might envision the reaction’s taking place by means of a collision between the molecules.
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
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?
7-35 A reaction has a high rate constant but a small equilibrium constant. What does this mean in terms of producing an industrial product?
The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?
By which of the following mechanisms does a catalyst operate? a. It decreases the activation energy barrier for a reaction. b. It serves as a reactant and is consumed. c. It increases the temperature of a reaction. d. It increases the concentration of reactants.
Chemical reactions occur when reactants collide. What are two factors that may prevent a collision from producing a chemical reaction?
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
How does an increase in temperature affect rate of reaction? Explain this effect in terms of the collision theory of the reaction rate.
For each of the following pairs of reaction diagrams, identify which of the pair is catalyzed:
Explain what is meant by the average rate of a reaction.