Question

For the following redox reaction, answer the questions below:

2 AgNO3 (aq) + Mg(s) 2 Ag(s) + Mg(NO3)2(aq)

• Identify the oxidation number of each element or ion by writing it the spaces below each species in the reaction above.

• What species was oxidized?

• What species was reduced?

• What substance is the oxidizing agent?

• What substance is the reducing agent?

Answer 1

Given reaction is

2AgNO3(aq) + Mg(s) ---------> 2Ag(s) + Mg(NO3)2(aq)

=> The oxidation state of Ag in AgNO3 is +1, and NO3 has -1 charge.

=> Mg(s) has 0 oxidation state and Ag(s) has zero oxidation state. And Mg in Mg(NO3)2 is +2 and NO3 has -1.

=> The species which increase their oxidation state are called oxidesed and the species which decrease their oxidation state are called reduced species.

=> The compound which is used to reduce the other compound is called reducing agent and the compound which is used to oxidise the other compound is called oxidising agent.

=> Here Ag in AgNO3 reduced from +1 to 0, so Ag is reduced and it is used as oxidising agent to oxidise Mg from 0 to +2.

=> Here Mg is increased oxidation state from 0 to +2, so it is oxidised and it is used as reducing agent to reduce Ag from +1 to 0.

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