Question

Use the changes in oxidation numbers to identify which atom is oxidized and which is

reduced. Then, determine which reactant is the oxidizing agent and which is the reducing
agent. (Show your work.).
a. H2 + Cl2 → 2 HCl
Oxidized ----------------------------------------- Reduced --------------------------------------------
Oxidizing Agent -------------------------------- Reducing Agent ----------------------------------

Answer 1

Oxidized: Hydrogen

Reduced: Chlorine

Oxidizing agent: Chlorine

Reducing agent: Hydrogen

Step-by-step explanation:

To determine which atom is oxidized and which is reduced, we need to compare the oxidation numbers of the atoms in the reactants and products.

In the reaction H2 + Cl2 → 2 HCl, the oxidation state of hydrogen in H2 is 0, while the oxidation state of chlorine in Cl2 is also 0. In the product HCl, the oxidation state of hydrogen is +1, while the oxidation state of chlorine is -1.

So, in this reaction, hydrogen is oxidized (its oxidation state increases from 0 to +1), while chlorine is reduced (its oxidation state decreases from 0 to -1).

To determine which reactant is the oxidizing agent and which is the reducing agent, we need to look at which reactant caused the oxidation and which caused the reduction.

In this case, chlorine caused the oxidation of hydrogen and is therefore the oxidizing agent. Hydrogen caused the reduction of chlorine and is therefore the reducing agent.