The rate of reaction is expressed as+frac{1}{ | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) For a general reaction $aA + bB 	o cC + dD$,the rate of reaction is expressed as:Rate $= -\frac{1}{a}\frac{d[A]}{dt} = -\frac{1}{b}\frac{d[B]}{dt

Vedclass · Accepted Answer

$B + 3D 	o 4A + 2C$

Vedclass · Answer

(C) For a general reaction $aA + bB 	o cC + dD$,the rate of reaction is expressed as:Rate $= -\frac{1}{a}\frac{d[A]}{dt} = -\frac{1}{b}\frac{d[B]}{dt} = +\frac{1}{c}\frac{d[C]}{dt} = +\frac{1}{d}\frac{d[D]}{dt}$Given expression:$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$Comparing the coefficients:For $C$,the coefficient is $2$.For $D$,the coefficient is $3$ (negative sign indicates reactant).For $A$,the coefficient is $4$.For $B$,the coefficient is $1$ (negative sign indicates reactant).Thus,the reactants are $B$ and $D$ with stoichiometric coefficients $1$ and $3$ respectively,and the products are $A$ and $C$ with stoichiometric coefficients $4$ and $2$ respectively.The balanced chemical equation is: $B + 3D 	o 4A + 2C$.

The rate of reaction is expressed as
$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$
The reaction is:

Similar Questions

For the reaction $2N_2O_{5(g)} \rightleftharpoons 4NO_{2(g)} + O_{2(g)}$ in a closed vessel,the concentration of $NO_2$ increases by $2.0 \times 10^{-2} \, mol \, L^{-1}$ in $5 \, s$. Calculate the rate of reaction.

Find the rate of the following reaction: $2 \ N_2O_{5(g)} \rightarrow 4 \ NO_{2(g)} + O_{2(g)}$ if the concentration of $NO_2$ increases to $5.2 \times 10^{-3} \ M$ in $100 \ s$.

Which one of the following equations is correct for the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$?

What is the rate of disappearance of $B$ in the following reaction? $2A + B \rightarrow 3C$,if the rate of appearance of $C$ is $1.3 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$.

For the reaction ${N_2}_{(g)} + 3{H_2}_{(g)} \to 2N{H_3}_{(g)}$,what is the relationship between $\frac{d[N{H_3}]}{dt}$ and $-\frac{d[{H_2}]}{dt}$?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

The rate of reaction is expressed as$+\frac{1}{2}\frac{d[C]}{dt} = -\frac{1}{3}\frac{d[D]}{dt} = +\frac{1}{4}\frac{d[A]}{dt} = -\frac{d[B]}{dt}$The reaction is: