Identify which of the following are redox reactions. If a reaction is a redox reaction, name the element oxidized, the element reduced, the oxidizing agent, and the reducing agent. a. Mg(s) + Br2(l) > MgBr2(s) b. H2CO3(aq) > H2O(l) + CO2(g)

The answer to your question is below

Explanation:

a.                   Mg(s) + Br₂(l) > MgBr₂(s)    It is a Redox reaction

- Calculate the Oxidation numbers

                     Mg(s)⁰ + Br₂(l)⁰ > Mg⁺²Br₂⁻¹(s)  

                                    Mg⁰    Mg⁺²      Reducing agent

                                    Br₂⁰ Br₂⁻¹        Oxidizing agent

b.                   H₂CO₃(aq) > H₂O(l) + CO₂(g)  It is not a Redox reaction

Calculate the oxidation numbers

                   H₂⁺¹C⁺⁴O₃⁻²(aq) > H₂⁺¹O⁻²(l) + C⁺⁴O₂⁻⁴(g)

n+h→nh3

we must remember that nitrogen and hydrogen are both diatomic molecules in their standard gas form. this adjusts the equation to

n2+h2→nh3

now we need to adjust coefficients in order to balance the atoms on each side of the equation. currently we have 2 atoms of nitrogen and 2 atoms of hydrogen on the reactant side and 1 atom of nitrogen and 3 atoms of hydrogen on the product side.

we can balance the hydrogens by placing a coefficient of 2 in front of ammonia and a coefficient of 3 in front of the hydrogen.

n2+3h2→2nh3

this gives us 6 hydrogen on each side and coincidentally the nitrogens now equal 2 on each side.