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

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(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

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

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(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:

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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: