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Ch.14 - Chemical Kinetics
All textbooksTro 4th EditionCh.14 - Chemical KineticsProblem 25c
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Chapter 14, Problem 25c

Consider the reaction:
2 HBr (g) → H2 (g) + Br2 (g)
c. If the volume of the reaction vessel in part b was 1.50 L, what amount of Br2 (in moles) was formed during the first 15.0 s of the reaction?

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1
Identify the balanced chemical equation for the reaction: 2 HBr (g) → H2 (g) + Br2 (g). This indicates that 2 moles of HBr produce 1 mole of Br2.
Determine the rate of the reaction from the given information or previous parts of the problem. The rate will tell you how much HBr is being consumed over a certain period.
Calculate the amount of HBr consumed in the first 15.0 seconds using the rate of the reaction.
Use the stoichiometry of the reaction from the balanced equation to find the amount of Br2 formed. Since 2 moles of HBr produce 1 mole of Br2, divide the moles of HBr consumed by 2 to get the moles of Br2 formed.
Ensure the units are consistent and the calculations are correct to find the moles of Br2 produced in the given time frame.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the relationships between the quantities of substances involved in a reaction, such as how many moles of one substance are produced from a given amount of another. In this case, understanding the stoichiometric coefficients from the reaction equation is essential to calculate the amount of Br2 formed.
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Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is crucial for understanding how gases behave under different conditions and can be used to calculate the number of moles of a gas when the volume and other parameters are known. In this question, it may be necessary to apply this law to find the moles of Br2 produced in the given volume.
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Reaction Rate

Reaction rate refers to the speed at which reactants are converted into products in a chemical reaction. It can be influenced by various factors, including concentration, temperature, and the presence of catalysts. In this scenario, knowing the reaction rate is important to determine how much Br2 is formed over a specific time period, which is 15.0 seconds in this case.
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Related Practice
Open Question
Cyclopropane (C3H6) reacts to form propene (C3H6) in the gas phase. The reaction is first order in cyclopropane and has a rate constant of 5.87 * 10^-4 s^-1 at 485 °C. If a 2.5-L reaction vessel initially contains 722 torr of cyclopropane at 485 °C, how long will it take for the partial pressure of cyclopropane to drop to below 1.00 * 10^2 torr?
Textbook Question

Consider the reaction:

2 HBr (g) → H2 (g) + Br2 (g)

a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products.

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Textbook Question

Consider the reaction:

2 HBr (g) → H2 (g) + Br2 (g)

b. In the first 25.0 s of this reaction, the concentration of HBr dropped from 0.600 M to 0.512 M. Calculate the average rate of the reaction during this time interval.

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Open Question
Consider the reaction: 2 N2O(g) → 2 N2(g) + O2(g). In the first 15.0 s of the reaction, 0.015 mol of O2 is produced in a reaction vessel with a volume of 0.500 L. a. What is the average rate of the reaction during this time interval? b. Predict the rate of change in the concentration of N2O during this time interval, i.e., what is ∆[N2O]/∆t?
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