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Br- and BrO...

Question

$B r^{-}$ and $B r O_{x}^{-}$ in acidic medium forms $B r_{2}$ , where x =

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Solution

Balanced reaction:

$5 B r^{-} + B r O_{3}^{-} + 6 H^{+} ⟶ 3 B r_{2} + 3 H_{2} O$
-1 +5 0

Value of x is 3.

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Similar questions

Q. Not balanced reaction

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

in acidic medium shows comproportionation to form Bromine. After balancing, x= no. of moles of

B r_{2}

produced, y= no. of moles of

B r O_{3}^{-}

used. The value of

\frac{x}{y} =

B r O_{3}^{-}

ion reacts with

{B r}^{-}

in acidic medium,

{B r}_{2}

is liberated. The equivalent weight

{B r}_{2}

in this reaction is :

Q. In acidic medium the rate of reaction between

(B r O_{3})^{-} a n d B r^{-}

ion is given by the expression

\frac{d [B r O_{3}^{-}]}{d t} = k [B r O_{3}^{-}] [B r^{-}] {[H^{+}]}^{2}

{B r O}_{3}^{-}

ion reacts with

{B r}^{-}

in acid medium,

{B r}_{2}

is liberated. The equivalent weight of

{B r}_{2}

in this reaction is:

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

(acidic) is a balanced equation.
If true enter 1, else enter 0.

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