Question

In the following equation, which element is oxidized and which element is reduced?

SN₂+ + 2 Ag → Sn + 2 Ag+
1) SN₂+ is oxidized and Ag is reduced
2) Sn is oxidized and Ag+ is reduced
3) Sn is oxidized and Ag is reduced
4) SN₂+ is oxidized and Ag+ is reduced

Answer 1

In the reaction Sn²⁺ + 2 Ag → Sn + 2 Ag⁺, Sn²⁺ is oxidized as it loses electrons, and Ag is reduced as it gains electrons. Therefore, Sn²⁺ is the reducing agent and Ag is the oxidizing agent.

Step-by-step explanation:

In the oxidation-reduction reaction Sn²⁺ + 2 Ag → Sn + 2 Ag⁺, we have to identify which element is oxidized and which is reduced. To do this, we look at the change in oxidation states for the elements involved. Sn²⁺ is oxidized because it goes from a +2 oxidation state to a 0 oxidation state by losing two electrons. Conversely, Ag is reduced because it goes from a 0 oxidation state to a +1 oxidation state by gaining an electron.

Therefore, the correct answer is:
1) Sn²⁺ is oxidized because it loses electrons.
2) Ag is reduced because it gains electrons.