Question

What are the coefficients in front of NO₃⁻(aq) and mg(s) when the following redox equation is balanced in an acidic solution? ________ NO₃⁻(aq) ________ mg(s) → ________ no(g) ________ mg2 (aq)?

1) 2, 3
2) 2, 6
3) 3, 4
4) 3, 6

Answer 1

The coefficients in front of the NO₃⁻(aq) and mg(s) when balancing the given redox equation in an acidic solution are 2 for NO₃⁻ and 3 for Mg. These coefficients ensure both mass and charge conservation.So the correct option is 1.

Step-by-step explanation:

To determine the coefficients in front of the reactants and products in the redox reaction involving NO₃⁻(aq) and mg(s), we must balance the equation keeping in mind that mass and charge must be conserved. To balance a redox reaction in an acidic solution, we break it down into two half-reactions, balance each for mass and charge, and then combine them so that electrons are also balanced.

For Mg we have the half-reaction: Mg(s) → Mg²⁻(aq) + 2e⁻. For NO₃⁻ to NO(g), the half-reaction would be: NO₃⁻(aq) + 3e⁻ + 4H⁻(aq) → NO(g) + 2H₂O(l).

By balancing the number of electrons, we can see that the Mg half-reaction must produce twice as many electrons. Therefore, we multiply the NO₃⁻ half-reaction by 2 and the Mg half-reaction by 3. As a result, we get: 2 NO₃⁻ + 3 Mg → 2 NO + 3 Mg²⁻ + H₂O. This gives us the coefficients: 2 for NO₃⁻ and 3 for Mg, which corresponds to option 1.