18649
The conversion of \(Pb{O_2}\) to \(Pb{(N{O_3})_2}\)is
1 Oxidation
2 Reduction
3 Neither oxidation nor reduction
4 Both oxidation and reduction
Explanation:
(b)\(\mathop {Pb{O_2}}\limits^{ + 4\,\,\,\,\,\,\,\,\,\,\,} \to \mathop {Pb{{(N{O_3})}_2}}\limits^{ + 2\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \). In this reaction reduction occurs.
Redox Reactions
18650
In the course of a chemical reaction an oxidant
1 Loses electrons
2 Gains electrons
3 Both loses and gains electron
4 Electron change takes place
Explanation:
(b) Any substance which is capable of oxidising other substances and is capable of accepting/gaining electron during oxidation is called oxidising agent or oxidant.
Redox Reactions
18651
\(2CuI\, \to Cu + Cu{I_2}\), the reaction is
1 Redox
2 Neutralisation
3 Oxidation
4 Reduction
Explanation:
(a) \(\mathop {2CuI}\limits^{ + 1\,\,} \to \mathop {Cu}\limits^0 \,\, + \mathop {Cu{I_2}}\limits^{ + 2\,\,\,\,\,} \). Oxidation and Reduction both occur so the reaction is redox.
Redox Reactions
18652
\({H_2}S\) reacts with halogens, the halogens
1 Form sulphur halides
2 Are oxidised
3 Are reduced
4 None of these
Explanation:
(c)\({H_2}S + {X_2}(Cl,\,Br,\,I\, = X) \to 2HX + S\). Here the halogen are reduced.
Redox Reactions
18653
\({H_2}{O_2}\) reduces \({K_4}Fe{(CN)_6}\)
1 In neutral solution
2 In acidic solution
3 In non-polar solvent
4 In alkaline solution
Explanation:
(b) When \({H_2}{O_2}\) reduces with \({K_4}[Fe{(CN)_6}]\). It is present in acidic solution. \(2{K_4}[Fe{(CN)_6} + {H_2}S{O_4} + {H_2}{O_2} \to \) \(2{K_3}[Fe{(CN)_6}] + {K_2}S{O_4} + 2{H_2}O\)
18649
The conversion of \(Pb{O_2}\) to \(Pb{(N{O_3})_2}\)is
1 Oxidation
2 Reduction
3 Neither oxidation nor reduction
4 Both oxidation and reduction
Explanation:
(b)\(\mathop {Pb{O_2}}\limits^{ + 4\,\,\,\,\,\,\,\,\,\,\,} \to \mathop {Pb{{(N{O_3})}_2}}\limits^{ + 2\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \). In this reaction reduction occurs.
Redox Reactions
18650
In the course of a chemical reaction an oxidant
1 Loses electrons
2 Gains electrons
3 Both loses and gains electron
4 Electron change takes place
Explanation:
(b) Any substance which is capable of oxidising other substances and is capable of accepting/gaining electron during oxidation is called oxidising agent or oxidant.
Redox Reactions
18651
\(2CuI\, \to Cu + Cu{I_2}\), the reaction is
1 Redox
2 Neutralisation
3 Oxidation
4 Reduction
Explanation:
(a) \(\mathop {2CuI}\limits^{ + 1\,\,} \to \mathop {Cu}\limits^0 \,\, + \mathop {Cu{I_2}}\limits^{ + 2\,\,\,\,\,} \). Oxidation and Reduction both occur so the reaction is redox.
Redox Reactions
18652
\({H_2}S\) reacts with halogens, the halogens
1 Form sulphur halides
2 Are oxidised
3 Are reduced
4 None of these
Explanation:
(c)\({H_2}S + {X_2}(Cl,\,Br,\,I\, = X) \to 2HX + S\). Here the halogen are reduced.
Redox Reactions
18653
\({H_2}{O_2}\) reduces \({K_4}Fe{(CN)_6}\)
1 In neutral solution
2 In acidic solution
3 In non-polar solvent
4 In alkaline solution
Explanation:
(b) When \({H_2}{O_2}\) reduces with \({K_4}[Fe{(CN)_6}]\). It is present in acidic solution. \(2{K_4}[Fe{(CN)_6} + {H_2}S{O_4} + {H_2}{O_2} \to \) \(2{K_3}[Fe{(CN)_6}] + {K_2}S{O_4} + 2{H_2}O\)
18649
The conversion of \(Pb{O_2}\) to \(Pb{(N{O_3})_2}\)is
1 Oxidation
2 Reduction
3 Neither oxidation nor reduction
4 Both oxidation and reduction
Explanation:
(b)\(\mathop {Pb{O_2}}\limits^{ + 4\,\,\,\,\,\,\,\,\,\,\,} \to \mathop {Pb{{(N{O_3})}_2}}\limits^{ + 2\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \). In this reaction reduction occurs.
Redox Reactions
18650
In the course of a chemical reaction an oxidant
1 Loses electrons
2 Gains electrons
3 Both loses and gains electron
4 Electron change takes place
Explanation:
(b) Any substance which is capable of oxidising other substances and is capable of accepting/gaining electron during oxidation is called oxidising agent or oxidant.
Redox Reactions
18651
\(2CuI\, \to Cu + Cu{I_2}\), the reaction is
1 Redox
2 Neutralisation
3 Oxidation
4 Reduction
Explanation:
(a) \(\mathop {2CuI}\limits^{ + 1\,\,} \to \mathop {Cu}\limits^0 \,\, + \mathop {Cu{I_2}}\limits^{ + 2\,\,\,\,\,} \). Oxidation and Reduction both occur so the reaction is redox.
Redox Reactions
18652
\({H_2}S\) reacts with halogens, the halogens
1 Form sulphur halides
2 Are oxidised
3 Are reduced
4 None of these
Explanation:
(c)\({H_2}S + {X_2}(Cl,\,Br,\,I\, = X) \to 2HX + S\). Here the halogen are reduced.
Redox Reactions
18653
\({H_2}{O_2}\) reduces \({K_4}Fe{(CN)_6}\)
1 In neutral solution
2 In acidic solution
3 In non-polar solvent
4 In alkaline solution
Explanation:
(b) When \({H_2}{O_2}\) reduces with \({K_4}[Fe{(CN)_6}]\). It is present in acidic solution. \(2{K_4}[Fe{(CN)_6} + {H_2}S{O_4} + {H_2}{O_2} \to \) \(2{K_3}[Fe{(CN)_6}] + {K_2}S{O_4} + 2{H_2}O\)
18649
The conversion of \(Pb{O_2}\) to \(Pb{(N{O_3})_2}\)is
1 Oxidation
2 Reduction
3 Neither oxidation nor reduction
4 Both oxidation and reduction
Explanation:
(b)\(\mathop {Pb{O_2}}\limits^{ + 4\,\,\,\,\,\,\,\,\,\,\,} \to \mathop {Pb{{(N{O_3})}_2}}\limits^{ + 2\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \). In this reaction reduction occurs.
Redox Reactions
18650
In the course of a chemical reaction an oxidant
1 Loses electrons
2 Gains electrons
3 Both loses and gains electron
4 Electron change takes place
Explanation:
(b) Any substance which is capable of oxidising other substances and is capable of accepting/gaining electron during oxidation is called oxidising agent or oxidant.
Redox Reactions
18651
\(2CuI\, \to Cu + Cu{I_2}\), the reaction is
1 Redox
2 Neutralisation
3 Oxidation
4 Reduction
Explanation:
(a) \(\mathop {2CuI}\limits^{ + 1\,\,} \to \mathop {Cu}\limits^0 \,\, + \mathop {Cu{I_2}}\limits^{ + 2\,\,\,\,\,} \). Oxidation and Reduction both occur so the reaction is redox.
Redox Reactions
18652
\({H_2}S\) reacts with halogens, the halogens
1 Form sulphur halides
2 Are oxidised
3 Are reduced
4 None of these
Explanation:
(c)\({H_2}S + {X_2}(Cl,\,Br,\,I\, = X) \to 2HX + S\). Here the halogen are reduced.
Redox Reactions
18653
\({H_2}{O_2}\) reduces \({K_4}Fe{(CN)_6}\)
1 In neutral solution
2 In acidic solution
3 In non-polar solvent
4 In alkaline solution
Explanation:
(b) When \({H_2}{O_2}\) reduces with \({K_4}[Fe{(CN)_6}]\). It is present in acidic solution. \(2{K_4}[Fe{(CN)_6} + {H_2}S{O_4} + {H_2}{O_2} \to \) \(2{K_3}[Fe{(CN)_6}] + {K_2}S{O_4} + 2{H_2}O\)
18649
The conversion of \(Pb{O_2}\) to \(Pb{(N{O_3})_2}\)is
1 Oxidation
2 Reduction
3 Neither oxidation nor reduction
4 Both oxidation and reduction
Explanation:
(b)\(\mathop {Pb{O_2}}\limits^{ + 4\,\,\,\,\,\,\,\,\,\,\,} \to \mathop {Pb{{(N{O_3})}_2}}\limits^{ + 2\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \). In this reaction reduction occurs.
Redox Reactions
18650
In the course of a chemical reaction an oxidant
1 Loses electrons
2 Gains electrons
3 Both loses and gains electron
4 Electron change takes place
Explanation:
(b) Any substance which is capable of oxidising other substances and is capable of accepting/gaining electron during oxidation is called oxidising agent or oxidant.
Redox Reactions
18651
\(2CuI\, \to Cu + Cu{I_2}\), the reaction is
1 Redox
2 Neutralisation
3 Oxidation
4 Reduction
Explanation:
(a) \(\mathop {2CuI}\limits^{ + 1\,\,} \to \mathop {Cu}\limits^0 \,\, + \mathop {Cu{I_2}}\limits^{ + 2\,\,\,\,\,} \). Oxidation and Reduction both occur so the reaction is redox.
Redox Reactions
18652
\({H_2}S\) reacts with halogens, the halogens
1 Form sulphur halides
2 Are oxidised
3 Are reduced
4 None of these
Explanation:
(c)\({H_2}S + {X_2}(Cl,\,Br,\,I\, = X) \to 2HX + S\). Here the halogen are reduced.
Redox Reactions
18653
\({H_2}{O_2}\) reduces \({K_4}Fe{(CN)_6}\)
1 In neutral solution
2 In acidic solution
3 In non-polar solvent
4 In alkaline solution
Explanation:
(b) When \({H_2}{O_2}\) reduces with \({K_4}[Fe{(CN)_6}]\). It is present in acidic solution. \(2{K_4}[Fe{(CN)_6} + {H_2}S{O_4} + {H_2}{O_2} \to \) \(2{K_3}[Fe{(CN)_6}] + {K_2}S{O_4} + 2{H_2}O\)
