For the reaction A+2B xrightarrow[] Products, the differential rate equation is

Question

For the reaction A+2B xrightarrow[] Products, the differential rate equation is (A)  -(1/2)(d[A]/dt)=(-d[B]/dt)=k[A][B]2  (B)  (1/2)-(d[A]/dt)=(d[B]/dt)=k[A][B]2  (C)  (-d[A]/dt)=-(1/2)(d[B]/dt)=k[A][B]2  (D)  (d[A]/dt)=(1/2)(d[B]/dt)=k[A][B]2

Tardigrade Admin · Accepted Answer

For the reaction A+2B xrightarrow products The differential rate equation is Rate =(-d[A]/dt)=-(1/2)(d[B]/dt) =k[A][B]2 where, k= rate constant.

Q. For the reaction $A + 2 B$ Products, the differential rate equation is

$- \frac{1}{2} \frac{d [ A ]}{d t} = \frac{- d [ B ]}{d t} = k [A] [B]^{2}$

$\frac{1}{2} - \frac{d [ A ]}{d t} = \frac{d [ B ]}{d t} = k [A] [B]^{2}$

$\frac{- d [ A ]}{d t} = - \frac{1}{2} \frac{d [ B ]}{d t} = k [A] [B]^{2}$

$\frac{d [ A ]}{d t} = \frac{1}{2} \frac{d [ B ]}{d t} = k [A] [B]^{2}$

For the reaction $A + 2 B$ products The differential rate equation is Rate $= \frac{- d [ A ]}{d t} = - \frac{1}{2} \frac{d [ B ]}{d t}$ $= k [A] [B] 2$ where, $k =$ rate constant.

Q. For the reaction A+2B​ Products, the differential rate equation is

−21​dtd[A]​=dt−d[B]​=k[A][B]2

21​−dtd[A]​=dtd[B]​=k[A][B]2

dt−d[A]​=−21​dtd[B]​=k[A][B]2

dtd[A]​=21​dtd[B]​=k[A][B]2