Consider the reaction: Cl2(g)+3 F2(g) ⟶2 ClF3(g) Complete the table. Δ[Cl2] / Δ t Δ[F2]

step 1 For the given chemical reaction where one mole of chlorine is reacting with three moles of fluor

Consider the reaction: Cl2(g)+3 F2(g) ⟶2 ClF3(g) Complete...

Consider the reaction: $\mathrm{Cl}_{2}(g)+3 \mathrm{~F}_{2}(g) \longrightarrow 2 \mathrm{ClF}_{3}(g)$ Complete the table. $$ \begin{array}{llll} \Delta\left[\mathrm{Cl}_{2}\right] / \Delta t & \Delta\left[\mathrm{F}_{2}\right] / \Delta t & \Delta\left[\mathrm{CIF}_{3}\right] / \Delta t & \text { Rate } \\ -0.012 \mathrm{M} / \mathrm{s} & \end{array} $$

Consider the reaction:
$\mathrm{Cl}_{2}(g)+3 \mathrm{~F}_{2}(g) \longrightarrow 2 \mathrm{ClF}_{3}(g)$
Complete the table.
$$
\begin{array}{llll}
\Delta\left[\mathrm{Cl}_{2}\right] / \Delta t & \Delta\left[\mathrm{F}_{2}\right] / \Delta t & \Delta\left[\mathrm{CIF}_{3}\right] / \Delta t & \text { Rate } \\
-0.012 \mathrm{M} / \mathrm{s} &
\end{array}
$$

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Key Concepts

Rate of Reaction

This concept refers to the speed at which reactants are converted into products in a chemical reaction. It is typically expressed as the change in concentration of a reactant or product per unit time. Understanding the rate of reaction is crucial for predicting how long a reaction will take to reach a certain extent and for controlling reaction conditions in industrial processes.

Stoichiometry

Stoichiometry involves the quantitative relationships among reactants and products in a chemical reaction. It uses the coefficients in a balanced chemical equation to relate the amounts of substances consumed and produced during the reaction. This concept is essential for determining how changes in the concentration of one species affect the others through their molar ratios.

Reaction Rates and Stoichiometric Coefficients

The relationship between the rate of change of concentrations and the stoichiometric coefficients in a balanced equation is a key concept in kinetics. For any chemical reaction, the rates of consumption or formation of each species are directly proportional to their stoichiometric coefficients. This allows for the conversion of the measured rate of one species into the corresponding rates for other species by applying the appropriate coefficients and sign conventions.

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