Consider the following reaction in aqueous solution. 5 Br -(a q)+ BrO 3 -(a q)+6 H +(a q) underset+3 H 2 O (l) longrightarrow If the rate of appearance of Br 2 at a particular moment during the reaction is 0.025 Ms -1, what is the rate of disappearance (in Ms -1 ) of Br -at that moment?

Question

Consider the following reaction in aqueous solution. 5 Br -(a q)+ BrO 3 -(a q)+6 H +(a q) underset+3 H 2 O (l) longrightarrow If the rate of appearance of Br 2 at a particular moment during the reaction is 0.025 Ms -1, what is the rate of disappearance (in Ms -1 ) of Br -at that moment? (A) 0.025 ms -1 (B) 0.042 ms -1 (C) 0.075 ms -1 (D) 0.125 ms -1

Tardigrade Admin · Accepted Answer

The two rates are related as .-(1/5) (d[ Br -]/d t)=(1/3) (d[ Br 2]/d t)] -(d[ Br -]/d t)=(5/3) (d[ Br 2]/d t) =(5/3) × 0.025=0.042 Ms -1

$0.025 m s^{- 1}$

$0.042 m s^{- 1}$

$0.075 m s^{- 1}$

$0.125 m s^{- 1}$

The two rates are related as
$- \frac{1}{5} \frac{d [ B r ^{-} ]}{d t} = \frac{1}{3} \frac{d [ B r _{2} ]}{d t}]$
$- \frac{d [ B r ^{-} ]}{d t} = \frac{5}{3} \frac{d [ B r _{2} ]}{d t}$
$= \frac{5}{3} \times 0.025 = 0.042 M s^{- 1}$

Q. Consider the following reaction in aqueous solution. 5Br−(aq)+BrO3​−(aq)+6H+(aq)+3H2​O(l)⟶​ If the rate of appearance of Br2​ at a particular moment during the reaction is 0.025Ms−1, what is the rate of disappearance (in Ms−1 ) of Br−at that moment?

0.025ms−1

0.042ms−1

0.075ms−1

0.125ms−1

The two rates are related as −51​dtd[Br−]​=31​dtd[Br2​]​] −dtd[Br−]​=35​dtd[Br2​]​ =35​×0.025=0.042Ms−1

$0.025 m s^{- 1}$

$0.042 m s^{- 1}$

$0.075 m s^{- 1}$

$0.125 m s^{- 1}$

The two rates are related as
$- \frac{1}{5} \frac{d [ B r ^{-} ]}{d t} = \frac{1}{3} \frac{d [ B r _{2} ]}{d t}]$
$- \frac{d [ B r ^{-} ]}{d t} = \frac{5}{3} \frac{d [ B r _{2} ]}{d t}$
$= \frac{5}{3} \times 0.025 = 0.042 M s^{- 1}$