When concentrated sulphuric acid is added to an inorganic mixture containing chloride, we get colourless pungent smell gas $H C l$ , but if the mixture contains bromide then we get red vapour of bromine. Why?

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Solution

$K B r + H_{2} S O_{4} \to K H S O_{4} + H B r$

HBr is a stronreducing agent which further reduces $H_{2} S O_{4}$ as follows
$2 H B r + H_{2} S O_{4} \to B r_{2} + S O_{2} + H_{2} O$
But in case of mixture containing Chloride the reaction end up on forming $H C l$ as $H C l$ is a weak reducing agent which can't further reduce
the sulphuric acid further.
$K C l + H_{2} S O_{4} \to K H S O_{4} + H C l colourless pungent smell gas$

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When concentrated sulphuric acid is added to an inorganic mixture containing chloride, we get colourless pungent smell gas HCl, but if the mixture contains bromide then we get red vapour of bromine. Why?

When concentrated sulphuric acid is added to an inorganic mixture containing chloride, we get colourless pungent smell gas $H C l$ , but if the mixture contains bromide then we get red vapour of bromine. Why?