A) \[NaBr+HCl\text{ }\xrightarrow{{}}NaCl+\text{ }HBr\]
B) \[HBr+AgN{{O}_{3}}\xrightarrow{{}}AgBr+HN{{O}_{3}}\]
C) \[{{H}_{_{2}}}+B{{r}_{2}}\xrightarrow{{}}2HBr\]
D) \[N{{a}_{2}}O+{{H}_{2}}S{{O}_{4}}\xrightarrow{{}}N{{a}_{2}}S{{O}_{4}}+{{H}_{2}}O\]
Correct Answer: C
Solution :
\[{{\overset{0}{\mathop{H}}\,}_{2}}+\overset{0}{\mathop{B{{r}_{2}}}}\,\xrightarrow{{}}\overset{+1-1}{\mathop{2HBr}}\,\] (0 to \[+1\]) increases the oxidation number of H in the reaction and (0 to \[-1\]) increases the oxidation number of Br in the reaction. So this is called redox reaction.
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