Difficult
Write the general reaction,its differential rate equation,and the rate law.
(N/A) General Reaction: $aA + bB \rightarrow cC + dD$ $(i)$
Where $a, b, c,$ and $d$ are the stoichiometric coefficients of reactants and products.
$(b)$ Rate Law: Rate $\propto [A]^{x} [B]^{y}$ or Rate $= k[A]^{x}[B]^{y}$ $(ii)$
Where $k$ is the rate constant,and $x$ and $y$ are the orders of reaction with respect to reactants $A$ and $B$,which may or may not be equal to the stoichiometric coefficients $a$ and $b$.
$(c)$ Differential Rate Equation: The rate of reaction can be expressed in terms of the change in concentration of reactants over time as:
Rate $= -\frac{d[R]}{dt} = k[A]^{x}[B]^{y}$
Example: For the reaction $2NO_{(g)} + O_{2(g)} \rightarrow 2NO_{2(g)}$,the rate law is Rate $= k[NO]^{2}[O_{2}]^{1}$.
Where $a, b, c,$ and $d$ are the stoichiometric coefficients of reactants and products.
$(b)$ Rate Law: Rate $\propto [A]^{x} [B]^{y}$ or Rate $= k[A]^{x}[B]^{y}$ $(ii)$
Where $k$ is the rate constant,and $x$ and $y$ are the orders of reaction with respect to reactants $A$ and $B$,which may or may not be equal to the stoichiometric coefficients $a$ and $b$.
$(c)$ Differential Rate Equation: The rate of reaction can be expressed in terms of the change in concentration of reactants over time as:
Rate $= -\frac{d[R]}{dt} = k[A]^{x}[B]^{y}$
Example: For the reaction $2NO_{(g)} + O_{2(g)} \rightarrow 2NO_{2(g)}$,the rate law is Rate $= k[NO]^{2}[O_{2}]^{1}$.
Explore More
Similar Questions
The experimental data for the reaction $2A + B_2 \longrightarrow 2AB$ is given below:
Exp. $[A] \ (mol \ L^{-1})$ $[B_2] \ (mol \ L^{-1})$ Rate $(mol \ L^{-1} \ S^{-1})$ $1$ $0.50$ $0.50$ $1.6 \times 10^{-4}$ $2$ $0.50$ $1.00$ $3.2 \times 10^{-4}$ $3$ $1.00$ $1.00$ $3.2 \times 10^{-4}$
Determine the rate law for the reaction.
| Exp. | $[A] \ (mol \ L^{-1})$ | $[B_2] \ (mol \ L^{-1})$ | Rate $(mol \ L^{-1} \ S^{-1})$ |
|---|---|---|---|
| $1$ | $0.50$ | $0.50$ | $1.6 \times 10^{-4}$ |
| $2$ | $0.50$ | $1.00$ | $3.2 \times 10^{-4}$ |
| $3$ | $1.00$ | $1.00$ | $3.2 \times 10^{-4}$ |
Determine the rate law for the reaction.
Difficult
View SolutionWhich of the following statements is correct?
Easy
View SolutionWhat is the order of the following reaction: $2H_2O_2(l) \rightarrow 2H_2O(l) + O_2(g)$, given that the rate law is $\text{rate} = k[H_2O_2]^1$?
For the reaction $H_{2(g)} + Br_{2(g)} \to 2HBr_{(g)}$,the experimental data suggest,$\text{rate} = K[H_2][Br_2]^{1/2}$. The molecularity and order of the reaction are respectively:
Easy
View Solution$2 \ NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2 \ NOCl_{(g)}$
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:
$Run$ $[NO]_{0}$ $[Cl_{2}]_{0}$ $r_{0}$ $1$ $0.10$ $0.10$ $0.18$ $2$ $0.10$ $0.20$ $0.35$ $3$ $0.20$ $0.20$ $1.40$
$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:
| $Run$ | $[NO]_{0}$ | $[Cl_{2}]_{0}$ | $r_{0}$ |
| $1$ | $0.10$ | $0.10$ | $0.18$ |
| $2$ | $0.10$ | $0.20$ | $0.35$ |
| $3$ | $0.20$ | $0.20$ | $1.40$ |
$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).
Vedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo