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.
Ch.14 - Chemical Kinetics
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?
Verified step by step guidance1
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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Stoichiometry Concept
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
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.
Textbook Question
Consider the reaction: 2 N2O( g) → 2 N2(g) + O2(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
For the reaction 2 A(g) + B(g) → 3 C(g), a. Determine the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products.