For the reaction 2 A(g)+B(g) ⟶3 C(g), a. determine the expression for the rate of the reaction

step 1 When the following reaction occurs, we can express the rate of reaction in terms of the change i

For the reaction 2 A(g)+B(g) ⟶3 C(g), a. determine the...

For the reaction $2 \mathrm{~A}(g)+\mathrm{B}(g) \longrightarrow 3 \mathrm{C}(g),$ a. determine the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products. b. when $A$ is decreasing at a rate of $0.100 \mathrm{M} / \mathrm{s},$ how fast is $\mathrm{B}$ decreasing? How fast is C increasing?

For the reaction $2 \mathrm{~A}(g)+\mathrm{B}(g) \longrightarrow 3 \mathrm{C}(g),$
a. determine the expression for the rate of the reaction in terms of the change in concentration of each of the reactants and products.
b. when $A$ is decreasing at a rate of $0.100 \mathrm{M} / \mathrm{s},$ how fast is $\mathrm{B}$ decreasing? How fast is C increasing?

Key Concepts

Relating Rates via Stoichiometric Coefficients

This key concept involves using the stoichiometric coefficients to convert the observed rate of change in one species to those of others. For instance, if one species is changing at a certain rate, the corresponding changes in other species can be determined by applying the ratio of the coefficients from the balanced equation, allowing for a comprehensive understanding of the reaction kinetics.

Sign Convention in Rate Expressions

This concept addresses the need to assign negative signs to the rates of change for reactants (which are being consumed) and positive signs for products (which are being formed). This convention is essential for accurately representing the dynamics of the reaction and ensuring consistency in the mathematical formulation of the rate laws.

Reaction Rate Expression

This concept involves expressing the rate of a reaction in terms of the changes in concentration of the reactants and products, normalized by their respective stoichiometric coefficients. It sets a framework for comparing how fast each species is consumed or produced during the reaction, typically leading to an equation where the reaction rate equals the negative change of reactant concentration divided by its coefficient or the positive change in product concentration divided by its coefficient.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products as given by the balanced chemical equation. In rate expressions, these coefficients determine the proportionality between the individual rates of change of concentrations, allowing one to relate the consumption of reactants to the formation of products during the reaction.

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