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Ch.15 - Chemical Kinetics
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.15 - Chemical KineticsProblem 90c
Chapter 15, Problem 90c

The tabulated data were collected for this reaction at a certain temperature: X2Y → 2 X + Y c. What is the concentration of X after 10.0 hours?

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Determine the rate law for the reaction. This involves understanding how the concentration of reactants affects the rate of the reaction.
Use the integrated rate law that corresponds to the order of the reaction. For example, if it's a first-order reaction, use the first-order integrated rate law: \( [A] = [A]_0 e^{-kt} \).
Identify the initial concentration of X, \([X]_0\), from the data provided.
Calculate the rate constant \(k\) using the data provided and the appropriate rate law.
Substitute the values of \([X]_0\), \(k\), and \(t = 10.0\) hours into the integrated rate law to find the concentration of X after 10.0 hours.

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Key Concepts

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

Chemical Reaction Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. In the given reaction, X<sub>2</sub>Y decomposes into 2 moles of X and 1 mole of Y, indicating the molar relationships between the substances. Understanding these ratios is essential for determining the concentration of products formed over time.
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Concentration and Molarity

Concentration refers to the amount of a substance in a given volume of solution, commonly expressed in molarity (moles per liter). To find the concentration of X after a specified time, one must consider the initial concentration of reactants and how they change as the reaction proceeds. This concept is crucial for quantifying the amount of X produced after 10.0 hours.
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Reaction Kinetics

Reaction kinetics studies the rates of chemical reactions and the factors affecting them. The time factor in the question (10.0 hours) is significant, as it influences how much of the reactants have converted into products. Understanding the kinetics of the reaction helps predict the concentration of X at a specific time point.
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Related Practice
Textbook Question

The tabulated data were collected for this reaction at 500 °C: CH3CN(g) → CH3NC( g) a. Determine the order of the reaction and the value of the rate constant at this temperature.

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Textbook Question

The activation barrier for the hydrolysis of sucrose into glucose and fructose is 108 kJ/mol. If an enzyme increases the rate of the hydrolysis reaction by a factor of 1 million, how much lower must the activation barrier be when sucrose is in the active site of the enzyme? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are identical and a temperature of 25 °C.)

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Textbook Question

Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 h at 25 °C. If a 1.5-L reaction vessel initially contains 745 torr of N2O5 at 25 °C, what partial pressure of O2 is present in the vessel after 215 minutes?

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