For the reaction 3Br O - - Br O 3 - -2 Br - in an alkaline aqueous solution- the value of the second order in Br O - rate constant at 80oC in the rate law for - Br O - - - t was found to be 0-056L mol -1 s -1- What is the rate constant when the rate law is written for a- Br O 3 - - - t -b- Br - - - t

3BrO^ → BrO^ _3 + 2Br^ Δ[BrO^ ]3dt = Δ[BrO^ _3]dt = Δ Br^ 2dt (i) #160; Δ[BrO^ _3]Δ t = 0.05^263 = 0.018 Lmol^ 1s^ 1 (ii) #160; ...

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

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

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

80

- \frac{Δ [{B r O}^{-}]}{Δ t}

L^{- 1} s - 1

\frac{Δ {B r O}_{3}^{-}}{Δ t}

\frac{Δ {B r}^{-}}{Δ t}

3 B r O^{-} ⟶ {B r O_{3}}^{-} + 2 {B r}^{-}

80^{o} C

- \frac{d}{d t} [B r O^{-}]

0.056

L

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

\frac{d}{d t} [{B r O_{3}}^{-}]

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

80^{\circ} C

- \frac{- d [B r O^{⊖}]}{d t}

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

\frac{d [B r O_{3}^{⊖}]}{d t}

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

= \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}

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

80^{\circ} C

- \frac{- d [B r O^{⊖}]}{d t}

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

\frac{d [B r O_{3}^{⊖}]}{d t}

5 B r^{- 1} (a q) + 6 H^{+} (a q) + B r O_{3}^{-} (a q) \to 3 B r_{2} (a q) + 3 H_{2} O (l)

- \frac{Δ [B r O_{3}^{-}]}{Δ t} = 0.01 m o l L^{- 1} m i n^{- 1}, \frac{Δ [B r_{2}]}{Δ t}

m o l L^{- 1} m i n^{- 1}

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