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. $4.8 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$

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Key Concepts

First Order Reactions

In first order reactions, the reaction rate is directly proportional to the concentration of one reactant, meaning the rate law takes the form Rate = k[A]. The understanding of first order processes includes using the integrated rate law to relate concentration changes over time.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction as given by the balanced equation. It is essential for converting changes in the concentration of one species to the corresponding changes in other species, based on their reaction coefficients.

Rate Constant

The rate constant is a numerical factor in the rate law that quantifies the speed of a reaction. It is dependent on temperature and the nature of the reaction, and for first order reactions it has units of s?¹, indicating the fraction of the reactant that reacts per second.

Reaction Kinetics

Reaction kinetics is the branch of chemistry that studies the rates of chemical processes and the factors that influence them. It focuses on how reactant concentrations, temperature, catalysts, and other conditions affect the speed at which a reaction proceeds.

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