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Home » Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions: (a) (b) (c) (d) (e)
Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions: (a) 2 \mathrm{AgBr}_{(s)}+\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{Ag}_{(s)}+2 \mathrm{HBr}_{(\mathrm{aq})}+\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{O}_{2}(\mathrm{aq}) (b) H C H O_{(l)}+2\left[A g\left(N H_{3}\right)_{2}\right]_{(a q)}^{+}+3 O H_{(a q)}^{-} \rightarrow 2 A g_{(s)}+H C O O_{(a q)}^{-}+ 4 \mathrm{NH}_{3}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}_{(l)} (c) \mathrm{HCHO}_{(l)}+2 \mathrm{Cu}_{(a q)}^{2+}+5 \mathrm{OH}_{(a q)}^{-} \rightarrow \mathrm{Cu}_{2} \mathrm{O}_{(s)}+\mathrm{HCOO}_{(a q)}^{-}+3 \mathrm{H}_{2} \mathrm{O}_{(l)} (d) N_{2} H_{4(l)}+2 \mathrm{H}_{2} \mathrm{O}_{2}(l) \rightarrow N_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}_{(l)} (e) \mathrm{Pb}_{(s)}+\mathrm{PbO}_{2(s)}+2 \mathrm{H}_{2} \mathrm{SO}_{4(a q)} \rightarrow 2 \mathrm{PbSO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}_{(l)}
CBSE | Chemistry | Class 11 | Exercise 1 | NCERT | Redox Reactions
Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions: (a) 2 \mathrm{AgBr}_{(s)}+\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{Ag}_{(s)}+2 \mathrm{HBr}_{(\mathrm{aq})}+\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{O}_{2}(\mathrm{aq}) (b) H C H O_{(l)}+2\left[A g\left(N H_{3}\right)_{2}\right]_{(a q)}^{+}+3 O H_{(a q)}^{-} \rightarrow 2 A g_{(s)}+H C O O_{(a q)}^{-}+ 4 \mathrm{NH}_{3}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}_{(l)} (c) \mathrm{HCHO}_{(l)}+2 \mathrm{Cu}_{(a q)}^{2+}+5 \mathrm{OH}_{(a q)}^{-} \rightarrow \mathrm{Cu}_{2} \mathrm{O}_{(s)}+\mathrm{HCOO}_{(a q)}^{-}+3 \mathrm{H}_{2} \mathrm{O}_{(l)} (d) N_{2} H_{4(l)}+2 \mathrm{H}_{2} \mathrm{O}_{2}(l) \rightarrow N_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}_{(l)} (e) \mathrm{Pb}_{(s)}+\mathrm{PbO}_{2(s)}+2 \mathrm{H}_{2} \mathrm{SO}_{4(a q)} \rightarrow 2 \mathrm{PbSO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}_{(l)}

Solution:

(a) 2 \mathrm{AgBr}_{(s)}+C_{6} H_{6} O_{2}(a q) \rightarrow 2 \mathrm{Ag}_{(s)}+2 \mathrm{HBr}_{(a q)}+C_{6} \mathrm{H}_{4} O_{2}(a q)

\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{2}=> Oxidized substance

\mathrm{AgBr}=> Reduced substance

\mathrm{AgBr}=> Oxidizing specialist

C_{6} H_{6} O_{2}=> Reducing specialist

(b) H C H O_{(l)}+2\left[A g\left(N H_{3}\right)_{2}\right]_{(a q)}^{+}+3 O H_{(a q)}^{-} \rightarrow 2 A g_{(s)}+H C O O_{(a q)}^{-}+

4 \mathrm{NH}_{3}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}_{(l)}

\mathrm{HCHO}=> Oxidized substance

\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+} \Rightarrow Reduced substance

\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+} \Rightarrow Oxidizing specialist

\mathrm{HCHO}=> Reducing specialist

(c) \mathrm{HCHO}_{(l)}+2 \mathrm{Cu}_{(a q)}^{2+}+5 \mathrm{OH}_{(a q)}^{-} \rightarrow \mathrm{Cu}_{2} \mathrm{O}_{(s)}+\mathrm{HCOO}_{(a q)}^{-}+3 \mathrm{H}_{2} \mathrm{O}_{(l)} \mathrm{HCHO}=> Oxidized substance

C u^{2+}=> Reduced substance

\mathrm{HCHO}=> Reducing specialist

(d) N_{2} H_{4}(l)+2 H_{2} O_{2}(l) \rightarrow N_{2}(g)+4 H_{2} O_{(t)}

N_{2} H_{4}=> Oxidized substance

\mathrm{H}_{2} \mathrm{O}_{2}=> Reduced substance

\mathrm{H}_{2} \mathrm{O}_{2}=> Oxidizing specialist

N_{2} H_{4}=> Reducing specialist

(e) \mathrm{Pb}_{(s)}+\mathrm{PbO}_{2(s)}+2 \mathrm{H}_{2} \mathrm{SO}_{4(a q)} \rightarrow 2 \mathrm{PbSO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}_{(l)}

\mathrm{Pb}=> Oxidized substance

\mathrm{PbO}_{2}=> Reduced substance

\mathrm{PbO}_{2}=> Oxidizing specialist

\mathrm{Pb}=> Reducing specialist

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