Show the balanced oxidation and reduction half – reactions UNDERLINE THE REDUCING AGENT and BOX THE...

Show the balanced oxidation and reduction half – reactions UNDERLINE THE REDUCING AGENT and BOX THE OXIDIZING AGENT in the final balanced equation:

NiO₂ (s) + Ag (s) ------> Ni²⁺ (aq) + Ag⁺ (aq) (Acidic Solution)

Solutions

Expert Solution

First, split the above equation in two parts and then balance individually and finally combine as:

NiO2 (s) ------> Ni2+ (aq) ------(1) and Ag (s) ------> Ag+ (aq) -------(2)

First balance eq (1) step by step as:

NiO2 (s) ------> Ni2+ (aq)

NiO2 (s) ------> Ni2+ (aq) + 2H2O (balance oxygen)

NiO2 (s) + 4H+ ------> Ni2+ (aq) + 2H2O (balance H)

NiO2 (s) + 4H+ + 2e- ------> Ni2+ (aq) + 2H2O (balance charge) ------(3)

Now, balance equation (2) as:

Ag (s) ------> Ag+ (aq)

Ag (s) ------> Ag+ (aq) + 1e- (balance charge) --------------(4)

Now, multiply eq (4) by 2 as:

2Ag (s) ------> 2Ag+ (aq) + 2e- ----------(5)

Finally, combine eq (3) and (5) as:

NiO2 (s) + 4H+ + 2e- + 2Ag (s) ------> Ni2+ (aq) + 2H2O + 2Ag+ (aq) + 2e-

Cancell the common electrons on either side to get balanced equation:

NiO2 (s) + 4H+ + 2Ag (s) ------> Ni2+ (aq) + 2Ag+ (aq) + 2H2O

Oxidizing agent NiO2 (as oxidation state of Ni decreases from +4 to +2).

Reducing agent Ag (as oxidation state increases from 0 to +1)

queen_honey_blossom answered 1 year ago

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