A chemical engineer is studying the rate of this reaction.H,CO, (aq) → H,O (aq)+CO, (aq)He fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds. Here's a graph of his data:[H2CO3] (M)0.8.0.60.4-0.200.020.040.060.080.10t (s)Use this graph to answer the following questions:What is the half life of the reaction?11/2= 0.03 s☐ x10Round your answer to 2 significant digits.Suppose the rate of the reaction is known to be first order inH2CO3. Calculate the value of the rate constant k.k == 0Round your answer to 2 significant digits. Also be sure youinclude the correct unit symbol.Predict the concentration of H2CO3 in the engineer'sreaction vessel after 0.150 seconds have passed.Assume no other reaction is important, and continue to[H,CO,] = Massume the rate is first order in H2CO3.Round your answer to 2 significant digits.☑

1. The half-life (t1/2) is the time it takes for the concentration of the reactant (H2CO3) to…

Answered: A chemical engineer is studying the…

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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Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
. Account for the increase in reaction rate brought about by a catalyst.
One of the concerns about the use of Freons is that they will migrate to the upper atmosphere, where chlorine atoms can be generated by the following reaction: CCl2F2(g)Freon-12hvCF2Cl(g)+Cl(g) Chlorine atoms can act as a catalyst for the destruction of ozone. The activation energy for the reaction Cl(g) + O3(g) ClO(g) + O2(g) Is 2.1 kJ/mol. Which is the more effective catalyst for the destruction of ozone, Cl or NO? (See Exercise 75.)
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.
Explain what is meant by the average rate of a reaction.
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
use the kineticmolecular theory to explain why an increase in temperature increases reaction rate.
. What does the activation energy for a reaction represent? How is the activation energy related to whether a collision between molecules is successful?
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?
Give at least two physical properties that might be used to determine the rate of a reaction.
A friend of yours states, A balanced equation tells us how chemicals interact. Therefore, we can determine the rate law directly from the balanced equations. What do you tell your friend?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.

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