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)

gas

explanation:

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given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g