18660
When copper turnings are added to silver nitrate solution, a blue coloured solution is formed after some time. It is because, copper
1 Displaces silver from the solution
2 Forms a blue coloured complex with \(AgN{O_3}\)
3 Is oxidised to \(C{u^{2 + }}\)
4 Is reduced to \(C{u^{2 + }}\)
Explanation:
(c) \(Cu\) is above of \(Ag\) in electrochemical series and thus \(Cu + 2A{g^ + } \to C{u^{2 + }} + 2Ag\) reaction occurs.
Redox Reactions
18661
Solution of sodium metal in liquid ammonia is strongly reducing due to the presence of the following in the solution
1 Sodium atoms
2 Solvated electrons
3 Sodium hydride
4 Sodium amide
Explanation:
of sodium metal in liquid ammonia is strongly reducing (reduction is gaining of electrons) due to the presence of solvated electrons (the solvated electrons supply electrons for reduction). A solvated electron is a free electron in a solution and is the smallest possible anion. Solvated electrons occur widely although they are often not observed directly. The deep color of solutions of alkali metals in ammonia arises from the presence of solvated electrons.
18660
When copper turnings are added to silver nitrate solution, a blue coloured solution is formed after some time. It is because, copper
1 Displaces silver from the solution
2 Forms a blue coloured complex with \(AgN{O_3}\)
3 Is oxidised to \(C{u^{2 + }}\)
4 Is reduced to \(C{u^{2 + }}\)
Explanation:
(c) \(Cu\) is above of \(Ag\) in electrochemical series and thus \(Cu + 2A{g^ + } \to C{u^{2 + }} + 2Ag\) reaction occurs.
Redox Reactions
18661
Solution of sodium metal in liquid ammonia is strongly reducing due to the presence of the following in the solution
1 Sodium atoms
2 Solvated electrons
3 Sodium hydride
4 Sodium amide
Explanation:
of sodium metal in liquid ammonia is strongly reducing (reduction is gaining of electrons) due to the presence of solvated electrons (the solvated electrons supply electrons for reduction). A solvated electron is a free electron in a solution and is the smallest possible anion. Solvated electrons occur widely although they are often not observed directly. The deep color of solutions of alkali metals in ammonia arises from the presence of solvated electrons.
18660
When copper turnings are added to silver nitrate solution, a blue coloured solution is formed after some time. It is because, copper
1 Displaces silver from the solution
2 Forms a blue coloured complex with \(AgN{O_3}\)
3 Is oxidised to \(C{u^{2 + }}\)
4 Is reduced to \(C{u^{2 + }}\)
Explanation:
(c) \(Cu\) is above of \(Ag\) in electrochemical series and thus \(Cu + 2A{g^ + } \to C{u^{2 + }} + 2Ag\) reaction occurs.
Redox Reactions
18661
Solution of sodium metal in liquid ammonia is strongly reducing due to the presence of the following in the solution
1 Sodium atoms
2 Solvated electrons
3 Sodium hydride
4 Sodium amide
Explanation:
of sodium metal in liquid ammonia is strongly reducing (reduction is gaining of electrons) due to the presence of solvated electrons (the solvated electrons supply electrons for reduction). A solvated electron is a free electron in a solution and is the smallest possible anion. Solvated electrons occur widely although they are often not observed directly. The deep color of solutions of alkali metals in ammonia arises from the presence of solvated electrons.
18660
When copper turnings are added to silver nitrate solution, a blue coloured solution is formed after some time. It is because, copper
1 Displaces silver from the solution
2 Forms a blue coloured complex with \(AgN{O_3}\)
3 Is oxidised to \(C{u^{2 + }}\)
4 Is reduced to \(C{u^{2 + }}\)
Explanation:
(c) \(Cu\) is above of \(Ag\) in electrochemical series and thus \(Cu + 2A{g^ + } \to C{u^{2 + }} + 2Ag\) reaction occurs.
Redox Reactions
18661
Solution of sodium metal in liquid ammonia is strongly reducing due to the presence of the following in the solution
1 Sodium atoms
2 Solvated electrons
3 Sodium hydride
4 Sodium amide
Explanation:
of sodium metal in liquid ammonia is strongly reducing (reduction is gaining of electrons) due to the presence of solvated electrons (the solvated electrons supply electrons for reduction). A solvated electron is a free electron in a solution and is the smallest possible anion. Solvated electrons occur widely although they are often not observed directly. The deep color of solutions of alkali metals in ammonia arises from the presence of solvated electrons.
