The decomposition of N2 O5 takes place according to I order as 2 N2 O5 ⟶4 NO2+O2 Calculate : (a

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The decomposition of N2 O5 takes place according to I order...

The decomposition of $\mathrm{N}_{2} \mathrm{O}_{5}$ takes place according to I order as $$ 2 \mathrm{~N}_{2} \mathrm{O}_{5} \longrightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2} $$ Calculate : (a) The rate constant, if instantaneous rate is $1.4 \times 10^{-6}$ mol litre $^{-1}$ $\mathrm{sec}^{-1}$ when concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ is $0.04 \mathrm{M}$ (b) The rate of reaction when concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ is $1.20 \mathrm{M}$ (c) The concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ when the rate of reaction will be $2.45 \times 10^{-5} \mathrm{~mol}$ litre $^{-1} \mathrm{sec}^{-\mathrm{i}}$.

The decomposition of $\mathrm{N}_{2} \mathrm{O}_{5}$ takes place according to I order as
$$
2 \mathrm{~N}_{2} \mathrm{O}_{5} \longrightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}
$$
Calculate :
(a) The rate constant, if instantaneous rate is $1.4 \times 10^{-6}$ mol litre $^{-1}$ $\mathrm{sec}^{-1}$ when concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ is $0.04 \mathrm{M}$
(b) The rate of reaction when concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ is $1.20 \mathrm{M}$
(c) The concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ when the rate of reaction will be $2.45 \times 10^{-5} \mathrm{~mol}$ litre $^{-1} \mathrm{sec}^{-\mathrm{i}}$.

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Key Concepts

Rate Law

The rate law is a mathematical expression that relates the rate of a chemical reaction to the concentration(s) of the reactant(s). It typically has the form rate = k[Reactant]^n, where k is the rate constant and n is the order of the reaction with respect to that reactant.

Rate Constant (k)

The rate constant is a proportionality constant in the rate law that quantifies the speed of the reaction. Its value depends on temperature and the specific reaction mechanism, and for a first-order reaction its units are reciprocal time (such as s?¹).

First-Order Kinetics

In a first-order reaction, the rate of reaction is directly proportional to the concentration of one reactant. This simplicity allows for easy calculation of reaction rates and concentration changes over time using the integrated first-order rate equation.

Instantaneous Rate

The instantaneous rate is the rate of reaction at a specific point in time, determined by the reaction conditions at that moment. It is used to calculate kinetic parameters by measuring the rate when the concentration of the reactant is known.

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