Question

The rate of a reaction is expressed in different ways as follows:

$+\frac{1}{2}\frac{d\left[C\right]}{dt}=-\frac{1}{3}\frac{d\left[D\right]}{dt}=+\frac{1}{4}\frac{d\left[A\right]}{dt}=-\frac{d\left[B\right]}{dt}$.

The reaction can be:

• A. $4A+B\to 2C+3D$
• B. $B+3D\to 4A+2C$
• C. $4A+2B\to 2C+3D$
• D. $B+\frac{1}{2}D\to 4A+3C$

Answer 1

Answer: (B)

$B+3D\to 4A+2C$

Explanation:

The rate which is given in negative sign that means that is the rate of reactant because the rate of reactant goes on decreasing in chemical reaction as reactant are consumed and product formation took place

Here $D$ and $B$ are reactant and $C$ and $A$ are products

write reaction with their stochiometric coefficient given

$Reactant\to Product$

$D+B\to A+C$

with their stochiometric coefficient reaction will be:

$3D+B\to 4A+2C$

Hence option B is correct answer