In the reaction, A+2 B → C+2D, the initial rate -d[A]/ dt at t=0 was found to be 2.6×10-2 M s-1. What is the value of -d [B] / dt at t=0 in Ms-1?

Question

In the reaction, A+2 B → C+2D, the initial rate -d[A]/ dt at t=0 was found to be 2.6×10-2 M s-1. What is the value of -d [B] / dt at t=0 in Ms-1? (A) 2.6×10-2 (B) 5.2×10-2 (C) 1.0×10-1 (D) 6.5×10-3

Tardigrade Admin · Accepted Answer

(d[A]/d t)=-(1/2) (d[B]/d t) Therefore, -(d[B]/d t)=2×(-d[A]/d t) =2×2.6×10-2 M s-1=5.2×10-2 M s-1

Q. In the reaction, $A + 2 B \to C + 2 D,$ the initial rate $- d [A] / d t a tt = 0$ was found to be $2.6 \times 1 0^{- 2} M s^{- 1} .$ What is the value of $- d [B] / d t a t t = 0 in M s^{- 1} ?$

$2.6 \times 1 0^{- 2}$

$5.2 \times 1 0^{- 2}$

$1.0 \times 1 0^{- 1}$

$6.5 \times 1 0^{- 3}$

$\frac{d [ A ]}{d t} = - \frac{1}{2} \frac{d [ B ]}{d t}$
$T h ere f ore, - \frac{d [ B ]}{d t} = 2 \times \frac{- d [ A ]}{d t}$
$= 2 \times 2.6 \times 1 0^{- 2} M s^{- 1} = 5.2 \times 1 0^{- 2} M s^{- 1}$

Q. In the reaction, A+2B→C+2D, the initial rate −d[A]/dtatt=0 was found to be 2.6×10−2Ms−1. What is the value of −d[B]/dtatt=0inMs−1?

2.6×10−2

5.2×10−2

1.0×10−1

6.5×10−3