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Ch.14 - Chemical Kinetics
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.14 - Chemical KineticsProblema 34c
Capitolo 14, Problema 34c

Consider the reaction: 2 H2O2(aq) → 2 H2O(l ) + O2( g) The graph shows the concentration of H2O2 as a function of time.
Use the graph to calculate each quantity: c. the instantaneous rate of formation of O2 at 50 s

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1
Determine the slope of the tangent line to the curve at 50 seconds on the graph of H_2O_2 concentration versus time.
Use the stoichiometry of the reaction: 2 H_2O_2(aq) → 2 H_2O(l) + O_2(g) to relate the rate of disappearance of H_2O_2 to the rate of formation of O_2.
The rate of formation of O_2 is half the rate of disappearance of H_2O_2, due to the stoichiometric coefficients in the balanced equation.
Calculate the instantaneous rate of formation of O_2 by taking half of the slope determined in the first step.
Express the rate in appropriate units, typically mol/L·s, based on the units used in the graph.

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Reaction Rate

The reaction rate refers to the speed at which reactants are converted into products in a chemical reaction. It can be expressed as the change in concentration of a reactant or product over time. Understanding how to calculate reaction rates is essential for analyzing chemical kinetics and determining how quickly a reaction proceeds.
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Average Rate of Reaction

Instantaneous Rate

The instantaneous rate of a reaction is the rate at a specific moment in time, rather than over an interval. It can be determined by taking the slope of the tangent line to the concentration vs. time graph at the desired time point. This concept is crucial for accurately assessing how fast a product is being formed or a reactant is being consumed at any given moment.
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Instantaneous Rate

Stoichiometry

Stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction, based on the balanced chemical equation. In the given reaction, the stoichiometric coefficients indicate that for every 2 moles of H2O2 decomposed, 1 mole of O2 is produced. This relationship is vital for converting the rate of formation of one substance into the rate of formation of another.
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Stoichiometry Concept
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