Which of the following reaction involves oxidation & reduction :-

N a B r + H C l \to N a C l + H B r

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H B r + {A g N O}_{3} \to A g B r + {H N O}_{3}

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2 N a O H + H_{2} {S O}_{4} \to {N a}_{2} {S O}_{4} + 2 H_{2} O

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H_{2} + {B r}_{2} \to 2 H B r

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Solution

The correct option is D $H_{2} + {B r}_{2} \to 2 H B r$
As refer to the above image here, hydrogen is oxidized from $0$ to $+ 1$ and bromine is reduced from $0$ to $- 1$ .

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Similar questions

H C l + N a O H \to N a C l + H_{2} O + x c a l .

H_{2} S O_{4} + 2 N a O H \to N a_{2} S O_{4} + 2 H_{2} O + y c a l

A g N O_{3} + N a B r \to N a N O_{3} + A g B r

B a C l_{2} + H_{2} S O_{4} \to B a S O_{4} + 2 H C l

A g N O_{3} + N a C l \to A g C l + N a N O_{3}

N a O H + H C l \to N a C l + H_{2} O

H C l + N a O H \to N a C l + H_{2} O + x c a l

H_{2} S O_{4} + 2 N a O H \to N a_{2} S O_{4} + 2 H_{2} O + y c a l

x

y

Balance the following chemical equations.

(a)

(b)

(c)

(d)

2 N a O H + H_{2} S O_{4} ⟶ N a_{2} S O_{4} + 2 H_{2} O

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