Ch.15 - Chemical Kinetics

Tro - Chemistry: A Molecular Approach 6th Edition

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Tro 6th Edition

Ch.15 - Chemical Kinetics

Problem 29a

Chapter 15, Problem 29a

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.

Verified step by step guidance

Start by understanding that the rate of a reaction is defined as the change in concentration of a reactant or product per unit time.

For the given reaction 2 A(g) + B(g) → 3 C(g), identify the stoichiometric coefficients: 2 for A, 1 for B, and 3 for C.

The rate of disappearance of a reactant is negative, while the rate of appearance of a product is positive.

Write the rate expression for each species: Rate = -\(\frac{1}{2}\)\(\frac{d[A]}{dt}\) = -\(\frac{d[B]}{dt}\) = \(\frac{1}{3}\)\(\frac{d[C]}{dt}\).

These expressions ensure that the rate of the reaction is the same regardless of which species' concentration change is being measured.

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Key Concepts

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

Rate of Reaction

The rate of a chemical reaction is a measure of how quickly reactants are converted into products. It is typically expressed as the change in concentration of a reactant or product per unit time. For a reaction, the rate can be influenced by factors such as temperature, concentration, and the presence of catalysts.

Stoichiometry

Stoichiometry involves the quantitative relationships between the amounts of reactants and products in a chemical reaction, as dictated by the balanced chemical equation. In the given reaction, the coefficients indicate the molar ratios of A, B, and C, which are essential for determining how changes in concentration affect the rate of the reaction.

Change in Concentration

The change in concentration refers to the difference in the concentration of a substance over a specific time interval. In the context of the reaction, it is crucial to express the rate in terms of the changes in concentration of both reactants and products, allowing for a comprehensive understanding of how the reaction progresses over time.

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Related Practice

Textbook Question

Consider the reaction: 8 H₂S(g) + 4 O₂(g) → 8 H₂O(g) + S₈(g) Complete the table.

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Textbook Question

Consider the reaction:

2 HBr (g) → H₂ (g) + Br₂ (g)

b. In the first 20.0 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 HBr (g) → H₂ (g) + Br₂ (g)

c. If the volume of the reaction vessel in part b was 1.25 L, what amount of Br₂ (in moles) was formed during the first 15.0 s of the reaction?

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(gg) + B(g) → 3 C(g), b. when A is decreasing at a rate of 0.200 M/s, how fast is B decreasing? How fast is C increasing?