In the reaction- 3Br O - -Br O 3 - -2 Br - aqueous alkaline medium at 80 o C the value of the rate constant in the rate law in terms of - d dt - Br O - - is 0-056 L mol -1 s -1- What will be the rate constant when the rate law is stated in terms of d dt - Br O 3 - -

The correct option is B 0.0187 L mol ^ 1 s ^ 1 1 3 d[ Br O ^ ] #160; dt = d[ Br O _ 3 ^ ] #160; dt =+ 1 2 d[ Br ^ ] #160; ...

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Byju's Answer

Standard XII

Chemistry

Factors Affecting Rate of Reaction

In the reacti...

Question

In the reaction, $3 B r O^{-} ⟶ {B r O_{3}}^{-} + 2 {B r}^{-}$ (aqueous alkaline medium at $80^{o} C$ ) the value of the rate constant in the rate law in terms of $- \frac{d}{d t} [B r O^{-}]$ is $0.056$ $L$ ${m o l}^{- 1} s^{- 1}$ . What will be the rate constant when the rate law is stated in terms of $\frac{d}{d t} [{B r O_{3}}^{-}]$ ?

18.7 \times 10^{- 3} L {m o l}^{- 1} s^{- 1}

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37.4 \times 10^{- 3} L {m o l}^{- 1} s^{- 1}

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0.0187 L {m o l}^{- 1} s^{- 1}

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18.7 \times 10^{- 2} L {m o l}^{- 1} s^{- 1}

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Solution

The correct option is B $0.0187 L {m o l}^{- 1} s^{- 1}$
$- \frac{1}{3} \frac{d [B r O^{-}]}{d t} = \frac{d [B r O_{3}^{-}]}{d t} = + \frac{1}{2} \frac{d [{B r}^{-}]}{d t}$
Required rate constant $= \frac{1}{3} \times 0.056$ $L$ ${m o l}^{- 1} s^{- 1}$
$= 0.0187$ $L$ ${m o l}^{- 1} s^{- 1}$

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Similar questions

Q. For the reaction

3 B r O^{-} \to B r O_{3}^{-} + 2 {B r}^{-}

in an alkaline aqueous solution, the value of the second order (in

B r O^{-}

rate constant at

80^{o} C

in the rate law for

- \frac{Δ [B r O^{-}]}{Δ t}

was found to be

0.056 L {m o l}^{- 1} s^{- 1}

. What is the rate constant when the rate law is written for

(a) \frac{Δ [B r O_{3}^{-}]}{Δ t}, (b) \frac{Δ [{B r}^{-}]}{Δ t}

Q. For reaction

3 B r O^{⊖} \to B r O_{3}^{⊖} + 2 B r^{⊖}

, the value of rate constant at

80^{\circ} C

in the rate for

- \frac{- d [B r O^{⊖}]}{d t}

was found to be

0.054 L m o l^{- 1} s^{- 1}

. The rate constant (k) for the reaction in terms of

\frac{d [B r O_{3}^{⊖}]}{d t}

is :

For the reaction :

a A + b B \to c C + d D

Rate

= \frac{d x}{d t} = \frac{- 1}{a} \frac{d [A]}{d t} = \frac{- 1}{b} \frac{d [B]}{d t} = \frac{- 1}{c} \frac{d [C]}{d t} = \frac{- 1}{d} \frac{d [D]}{d t}

For reaction

3 B r O^{⊖} \to B r O_{3}^{⊖} + 2 B r^{⊖}

, the value of rate constant at

80^{\circ} C

in the rate for

- \frac{- d [B r O^{⊖}]}{d t}

was found to be

0.054 L m o l^{- 1} s^{- 1}

. The rate constant (k) for the reaction in terms of

\frac{d [B r O_{3}^{⊖}]}{d t}

is :

Q. For the reaction

{3 B r O}^{-} \to {B r O}_{3}^{-} + {2 B r}^{-}

in an alkaline aquesous solution, the value of the second order

(i n {B r O}^{-})

rate at

80

in the rate law for

- \frac{Δ [{B r O}^{-}]}{Δ t}

was found to be 0.056 mol

L^{- 1} s - 1

. What is the rate when the rate law is written for (a)

\frac{Δ {B r O}_{3}^{-}}{Δ t}

,(b)

\frac{Δ {B r}^{-}}{Δ t}

Q. The rate of a first order reaction is

1.8 \times 10^{- 3} m o l L^{- 1} m i n^{- 1},

when the initial concentration is 0.3 mol

L^{- 1}

. The rate constant in the units of second is

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In the reaction, 3BrO−⟶BrO3−+2Br− (aqueous alkaline medium at 80oC) the value of the rate constant in the rate law in terms of −ddt[BrO−] is 0.056 L mol−1s−1. What will be the rate constant when the rate law is stated in terms of ddt[BrO3−]?

The correct option is B 0.0187 L mol−1s−1−13d[BrO−]dt=d[BrO−3]dt=+12d[Br−]dtRequired rate constant =13×0.056 L mol−1s−1 =0.0187 L mol−1s−1

The correct option is B $0.0187 L {m o l}^{- 1} s^{- 1}$
$- \frac{1}{3} \frac{d [B r O^{-}]}{d t} = \frac{d [B r O_{3}^{-}]}{d t} = + \frac{1}{2} \frac{d [{B r}^{-}]}{d t}$
Required rate constant $= \frac{1}{3} \times 0.056$ $L$ ${m o l}^{- 1} s^{- 1}$
$= 0.0187$ $L$ ${m o l}^{- 1} s^{- 1}$