which of the following are redox reactions

a. 2Na+2H2O-->2Naoh+H2
b. MgBr2+2NaF-->MgF2+2NaBr
c. 2CO+O2--> 2CO2
d. SO2+H2O--> H2SO3
For those reactions that are redox reactions:
Indicate which atoms get oxidized and which atoms get reduced.
Indicate which reactant is the oxidizing agent and which is the reducing agent.

Reduction half-reaction for 2Li(s)+2H+(aq)→2Li+(aq)+H2(g).

To determine which of the given reactions are redox reactions, we need to identify if there are any changes in the oxidation states of the atoms involved.

a. 2Na + 2H2O → 2NaOH + H2
This is a redox reaction as the oxidation state of sodium changes from 0 to +1, and the oxidation state of hydrogen changes from 0 to -1.

Oxidized: Hydrogen (H)
Reduced: Sodium (Na)

The oxidizing agent is water (H2O) because it causes a decrease in the oxidation state of hydrogen. The reducing agent is sodium (Na) because it causes an increase in the oxidation state of sodium.

b. MgBr2 + 2NaF → MgF2 + 2NaBr
This is not a redox reaction as there are no changes in the oxidation states of the atoms involved.

c. 2CO + O2 → 2CO2
This is a redox reaction as the oxidation state of carbon changes from +2 to +4, and the oxidation state of oxygen changes from 0 to -2.

Oxidized: Carbon (C)
Reduced: Oxygen (O)

The oxidizing agent is oxygen (O2) because it causes an increase in the oxidation state of carbon. The reducing agent is carbon monoxide (CO) because it causes a decrease in the oxidation state of oxygen.

d. SO2 + H2O → H2SO3
This is a redox reaction as the oxidation state of sulfur changes from +4 to +6, and the oxidation state of hydrogen changes from 0 to +1.

Oxidized: Sulfur (S)
Reduced: Hydrogen (H)

The oxidizing agent is water (H2O) because it causes an increase in the oxidation state of sulfur. The reducing agent is sulfur dioxide (SO2) because it causes a decrease in the oxidation state of hydrogen.

To determine whether each of the given reactions is a redox reaction, we need to compare the oxidation states of the atoms involved before and after the reaction.

A redox reaction involves a change in the oxidation states of the atoms. The reactant that gets oxidized loses electrons, and its oxidation state increases. The reactant that gets reduced gains electrons, and its oxidation state decreases.

Let's analyze each reaction:

a. 2Na + 2H2O --> 2NaOH + H2
In this reaction, sodium (Na) goes from an oxidation state of 0 to +1 in NaOH, indicating oxidation. Hydrogen (H) goes from an oxidation state of 0 to -1 in H2, indicating reduction. Therefore, this reaction is a redox reaction.
Na gets oxidized, and H gets reduced. The reactant Na is the reducing agent, and H2O is the oxidizing agent.

b. MgBr2 + 2NaF --> MgF2 + 2NaBr
In this reaction, the oxidation states of magnesium (Mg), bromine (Br), and fluorine (F) do not change. The reaction involves a simple exchange of ions. Since there is no change in oxidation states, this reaction is not a redox reaction.

c. 2CO + O2 --> 2CO2
In this reaction, carbon (C) goes from an oxidation state of +2 in CO to +4 in CO2, indicating oxidation. Oxygen (O) goes from an oxidation state of 0 to -2 in CO2, indicating reduction. Therefore, this reaction is a redox reaction.
C gets oxidized, and O gets reduced. The reactant CO is the reducing agent, and O2 is the oxidizing agent.

d. SO2 + H2O --> H2SO3
In this reaction, sulfur (S) goes from an oxidation state of +4 in SO2 to +6 in H2SO3, indicating oxidation. Hydrogen (H) goes from an oxidation state of +1 in H2O to 0 in H2SO3, indicating reduction. Therefore, this reaction is a redox reaction.
S gets oxidized, and H gets reduced. The reactant S0 is the reducing agent, and H2O is the oxidizing agent.

To summarize:
Redox reactions: a, c, and d
a. Oxidized: Na; Reduced: H
b. Not a redox reaction
c. Oxidized: C; Reduced: O
d. Oxidized: S; Reduced: H

a. Reducing agent: Na; Oxidizing agent: H2O
c. Reducing agent: CO; Oxidizing agent: O2
d. Reducing agent: SO2; Oxidizing agent: H2O

What is it you don't understand about these? I'm not a "do all your homework for you" person.