The rate constant for the reaction, 2 N2 O5 →4 NO2+O2 is 3.0 ×10^-4 s^-1. If start made with 1

step 1 in this problem as mole per liter of n205 reacted is equal to 2 multiplication 0 .1 which is equ

The rate constant for the reaction, 2 N2 O5 →4 NO2+O2 is...

The rate constant for the reaction, $2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}$ is $3.0 \times 10^{-4} \mathrm{~s}^{-1}$. If start made with $1.0 \mathrm{~mol} \mathrm{~L}^{-1}$ of $\mathrm{N}_{2} \mathrm{O}_{5}$, calculate the rate of formation of $\mathrm{NO}_{2}$ at the moment of the reaction when concentration of $\mathrm{O}_{2}$ is $0.1 \mathrm{~mol} \mathrm{~L}^{-1}$. a. $1.2 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ b. $3.6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ c. $9.6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ d. $4.8 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$

The rate constant for the reaction, $2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}$
is $3.0 \times 10^{-4} \mathrm{~s}^{-1}$. If start made with $1.0 \mathrm{~mol} \mathrm{~L}^{-1}$ of $\mathrm{N}_{2} \mathrm{O}_{5}$, calculate the rate of formation of $\mathrm{NO}_{2}$ at the moment of the reaction when concentration of $\mathrm{O}_{2}$ is $0.1 \mathrm{~mol} \mathrm{~L}^{-1}$.
a. $1.2 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$
b. $3.6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$
c. $9.6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$
d. $4.8 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$

Key Concepts

Stoichiometry in Kinetics

Stoichiometry in kinetics involves using the balanced chemical equation to connect the rates of consumption and production of various species in a reaction. By applying the stoichiometric coefficients, one can convert between the rate of decrease of one species and the rate of formation of another, which is particularly useful in calculating the formation rates of products from known reactant consumption rates.

First-Order Reaction

A first-order reaction is one where the rate of the reaction is directly proportional to the concentration of one reactant. This results in a simple rate law where the change in concentration over time depends linearly on the reactant’s concentration, simplifying the analysis and prediction of the reaction’s behavior over time.

Reaction Kinetics

Reaction kinetics studies the rates at which chemical processes occur and the factors that affect these speeds. It provides the framework for understanding how reactant concentrations change over time and how different reaction conditions (such as temperature or catalysts) influence the rate, which is crucial for both predicting and controlling chemical reactions.

Rate Constant

The rate constant is a proportionality factor in the rate law that quantifies the speed of a chemical reaction under a given set of conditions. It relates the concentrations of the reactants to the reaction rate and is essential in both differential and integrated rate laws, providing a measure of how quickly a reaction proceeds.

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