Justify that the following reactions are redox reactions:
$(a) \ CuO_{(s)} + H_{2(g)} \to Cu_{(s)} + H_2O_{(g)}$
$(b) \ Fe_2O_{3(s)} + 3CO_{(g)} \to 2Fe_{(s)} + 3CO_{2(g)}$
$(c) \ 4BCl_{3(g)} + 3LiAlH_{4(s)} \to 2B_2H_{6(g)} + 3LiCl_{(s)} + 3AlCl_{3(s)}$
$(d) \ 2K_{(s)} + F_{2(g)} \to 2K^+F^-_{(s)}$
$(e) \ 4NH_{3(g)} + 5O_{2(g)} \to 4NO_{(g)} + 6H_2O_{(g)}$
$(a) \ CuO_{(s)} + H_{2(g)} \to Cu_{(s)} + H_2O_{(g)}$
$(b) \ Fe_2O_{3(s)} + 3CO_{(g)} \to 2Fe_{(s)} + 3CO_{2(g)}$
$(c) \ 4BCl_{3(g)} + 3LiAlH_{4(s)} \to 2B_2H_{6(g)} + 3LiCl_{(s)} + 3AlCl_{3(s)}$
$(d) \ 2K_{(s)} + F_{2(g)} \to 2K^+F^-_{(s)}$
$(e) \ 4NH_{3(g)} + 5O_{2(g)} \to 4NO_{(g)} + 6H_2O_{(g)}$
(A) $(a) \ CuO_{(s)} + H_{2(g)} \to Cu_{(s)} + H_2O_{(g)}$
Oxidation number of $Cu$ decreases from $+2$ to $0$ (reduction) and $H$ increases from $0$ to $+1$ (oxidation). Thus,it is a redox reaction.
$(b) \ Fe_2O_{3(s)} + 3CO_{(g)} \to 2Fe_{(s)} + 3CO_{2(g)}$
Oxidation number of $Fe$ decreases from $+3$ to $0$ (reduction) and $C$ increases from $+2$ to $+4$ (oxidation). Thus,it is a redox reaction.
$(c) \ 4BCl_{3(g)} + 3LiAlH_{4(s)} \to 2B_2H_{6(g)} + 3LiCl_{(s)} + 3AlCl_{3(s)}$
Oxidation number of $B$ decreases from $+3$ to $-3$ (reduction) and $H$ increases from $-1$ to $+1$ (oxidation). Thus,it is a redox reaction.
$(d) \ 2K_{(s)} + F_{2(g)} \to 2K^+F^-_{(s)}$
Oxidation number of $K$ increases from $0$ to $+1$ (oxidation) and $F$ decreases from $0$ to $-1$ (reduction). Thus,it is a redox reaction.
$(e) \ 4NH_{3(g)} + 5O_{2(g)} \to 4NO_{(g)} + 6H_2O_{(g)}$
Oxidation number of $N$ increases from $-3$ to $+2$ (oxidation) and $O$ decreases from $0$ to $-2$ (reduction). Thus,it is a redox reaction.
Oxidation number of $Cu$ decreases from $+2$ to $0$ (reduction) and $H$ increases from $0$ to $+1$ (oxidation). Thus,it is a redox reaction.
$(b) \ Fe_2O_{3(s)} + 3CO_{(g)} \to 2Fe_{(s)} + 3CO_{2(g)}$
Oxidation number of $Fe$ decreases from $+3$ to $0$ (reduction) and $C$ increases from $+2$ to $+4$ (oxidation). Thus,it is a redox reaction.
$(c) \ 4BCl_{3(g)} + 3LiAlH_{4(s)} \to 2B_2H_{6(g)} + 3LiCl_{(s)} + 3AlCl_{3(s)}$
Oxidation number of $B$ decreases from $+3$ to $-3$ (reduction) and $H$ increases from $-1$ to $+1$ (oxidation). Thus,it is a redox reaction.
$(d) \ 2K_{(s)} + F_{2(g)} \to 2K^+F^-_{(s)}$
Oxidation number of $K$ increases from $0$ to $+1$ (oxidation) and $F$ decreases from $0$ to $-1$ (reduction). Thus,it is a redox reaction.
$(e) \ 4NH_{3(g)} + 5O_{2(g)} \to 4NO_{(g)} + 6H_2O_{(g)}$
Oxidation number of $N$ increases from $-3$ to $+2$ (oxidation) and $O$ decreases from $0$ to $-2$ (reduction). Thus,it is a redox reaction.
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Similar Questions
Which of the following shows a metal being oxidised?
Medium
View SolutionWhich one is the oxidising agent in the reaction below?
$2CrO_4^{2-} + 2H^{+} \to Cr_2O_7^{2-} + H_2O$
$2CrO_4^{2-} + 2H^{+} \to Cr_2O_7^{2-} + H_2O$
Easy
View SolutionWhich of the following is not correct?
Match each of the reactions given in Column $I$ with the corresponding product$(s)$ given in Column $II$.
Column $I$ Column $II$ $(A)$ $Cu + \text{dil } HNO_3$ $(p)$ $NO$ $(B)$ $Cu + \text{conc } HNO_3$ $(q)$ $NO_2$ $(C)$ $Zn + \text{dil } HNO_3$ $(r)$ $N_2O$ $(D)$ $Zn + \text{conc } HNO_3$ $(s)$ $Cu(NO_3)_2$ $(t)$ $Zn(NO_3)_2$
| Column $I$ | Column $II$ |
| $(A)$ $Cu + \text{dil } HNO_3$ | $(p)$ $NO$ |
| $(B)$ $Cu + \text{conc } HNO_3$ | $(q)$ $NO_2$ |
| $(C)$ $Zn + \text{dil } HNO_3$ | $(r)$ $N_2O$ |
| $(D)$ $Zn + \text{conc } HNO_3$ | $(s)$ $Cu(NO_3)_2$ |
| $(t)$ $Zn(NO_3)_2$ |
Which of the following are non-metal displacement reactions?
$(A)$ $Ca_{(s)} + 2 H_2 O_{(l)} \longrightarrow Ca(OH)_{2(aq)} + H_{2(g)}$
$(B)$ $V_2 O_{5(s)} + 5 Ca_{(s)} \stackrel{\Delta}{\longrightarrow} 2 V_{(s)} + 5 CaO_{(s)}$
$(C)$ $2 Fe_{(s)} + 3 H_2 O_{(g)} \stackrel{\Delta}{\longrightarrow} Fe_2 O_{3(s)} + 3 H_{2(g)}$
$(D)$ $Cr_2 O_{3(s)} + 2 Al_{(s)} \stackrel{\Delta}{\longrightarrow} Al_2 O_{3(s)} + 2 Cr_{(s)}$
$(A)$ $Ca_{(s)} + 2 H_2 O_{(l)} \longrightarrow Ca(OH)_{2(aq)} + H_{2(g)}$
$(B)$ $V_2 O_{5(s)} + 5 Ca_{(s)} \stackrel{\Delta}{\longrightarrow} 2 V_{(s)} + 5 CaO_{(s)}$
$(C)$ $2 Fe_{(s)} + 3 H_2 O_{(g)} \stackrel{\Delta}{\longrightarrow} Fe_2 O_{3(s)} + 3 H_{2(g)}$
$(D)$ $Cr_2 O_{3(s)} + 2 Al_{(s)} \stackrel{\Delta}{\longrightarrow} Al_2 O_{3(s)} + 2 Cr_{(s)}$
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