Question

Complete and balance the following reaction, assuming an acidic environment, by filling in the missing coefficients and formulas.

Ag(s)+NO−3(aq)⟶Ag+(aq)+NO₂(g)

Answer 1

To balance the reaction Ag(s) + NO3−(aq) ⟶ Ag+(aq) + NO2(g) in an acidic environment, we must consider the oxidation of Ag and the reduction of NO3−. The balanced equation in an acidic environment is given by 3 Ag(s) + NO3−(aq) + 4H+(aq) ⟶ 3 Ag+(aq) + NO2(g) + 2H2O(l).

Step-by-step explanation:

To complete and balance the chemical reaction Ag(s) + NO3−(aq) ⟶ Ag+(aq) + NO2(g) in an acidic environment, we first recognize that silver (Ag) is oxidized to silver ions (Ag+), while the nitrate ion (NO3−) is reduced to nitrogen dioxide (NO2). Since the environment is acidic, we can use H+ ions and water to balance hydrogen and oxygen atoms.

The half-reactions for the process are:

• Oxidation: Ag(s) ⟶ Ag+(aq) + e−
• Reduction: NO3− + 4H+ + 3e− ⟶ NO2(g) + 2H2O(l)

Since the reduction half-reaction requires 3 electrons and the oxidation provides only 1, we need to multiply the oxidation half-reaction by 3 to match the number of electrons:

• 3 Ag(s) ⟶ 3 Ag+(aq) + 3e−

Adding the two half-reactions gives us the balanced equation:

3 Ag(s) + NO3−(aq) + 4H+ ⟶ 3 Ag+(aq) + NO2(g) + 2H2O(l)