How do you solve this?

Question

Are any of these equations redox reactions? if so what are their reducing and oxidizing agents?

Na2CO3(s)+H3PO4(aq)→Na2HPO4(aq)+CO2(g)+H2O(l)

2Na(s)+Cl2(g)→2NaCl(s)



FeO(s)+CO(g)→Fe(s)+CO2(g)

Answer 1

Are any of these equations redox reactions? if so what are their reducing and oxidizing agents?

Find the oxidation numbers of all reactants and products.

If the oxidation numbers, change, it’s redox. IF they don’t change, not redox.

The oxidized reactant is the reducing agent.

The reduced reactant is the oxidizing agent.

Na2CO3(s)+H3PO4(aq)→Na2HPO4(aq)+CO2(g)+H2O(l)

Double replacement reactions are never redox.

On both sides, reactants and products:

Na=+1

C=+4

O=-2

P=+5

H=+1

2Na(s)+Cl2(g)→2NaCl(s)



Reactants: Na0, Cl0

Products: Na+, Cl-

Oxidation half rxn: Na0 → Na+ + e-

Reduction half rxn: Cl2+2e-→2Cl-

Na is oxidized, Cl2 is reduced

Na is reducing agent

Cl2 is oxidizing agent

FeO(s)+CO(g)→Fe(s)+CO2(g)

Reactants: Fe2+, O2-, C2+, O2-

Products: Fe0, C4+, O2-

Ox half rxn: C2+ → C4++2e-

Red half rxn: Fe2++2e- → Fe

C2+ is oxidized, Fe2+ is reduced

CO is reducing agent FeO is oxidizing agent