In the following disproportionation of }Cl_2 in basic } medium:- }{Cl_2+2KOH→ KCl+KClO+H_2O}; equivalent mass of }Cl_2 is } (a) }35.50 (b) }71.00 (c) }47.33 (d) }11.83

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Q. From the following reaction sequences, the mass of

{C l}_{2}

needed to produce

100

g of

K C l O_{4}

is (as the nearest integer) :

{C l}_{2} + 2 K O H \to K C l + K C l O + H_{2} O . . . (i)

3 K C l O \to 2 K C l + K C l O_{3} . . . (i i)

4 K C l O_{3} \to 3 K C l O_{4} + K C l . . . (i i i)

Q. Balance the following disproportionation reaction.

C l_{2} + K O H \to K C l O_{3} + K C l + H_{2} O

K_{2} {C r}_{2} O_{7} + H C l \to C r {C l}_{3} + H_{2} O + {C l}_{2} + K C l

Balance in basic medium by ion-electron identity spectator ion.

From the following reaction sequence
$C l_{2}$ + 2KOH $\to$ KCl + KClO + $H_{2} O$
3KClO $\to$ 2KCl + $K C l O_{3}$
$4 K C l O_{3}$ $\to$ $3 K C l O_{4} + K C l$

Calculate the mass of chlorine needed to produce 100g of $K C l O_{4}$

C l_{2}

disproportionate to

C l^{-}

and species

A

, such that the equivalent mass of

C l_{2}

71

. Thus, the oxidation number of chlorine in species

A

is:

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