Identify which substances are oxidized and which are reduced for the following reaction.
Zn + 2HCl = H2 + ZnCl2
Zn is oxidized and H+1 is reduced.
In the given reaction, Zn (zinc) reacts with HCl (hydrochloric acid) to produce H2 (hydrogen gas) and ZnCl2 (zinc chloride).
To determine which substances are oxidized and reduced, we need to look at the changes in their oxidation states.
Oxidation refers to the loss of electrons or an increase in oxidation state, while reduction refers to the gain of electrons or a decrease in oxidation state.
Let's analyze the oxidation states before and after the reaction:
Zinc (Zn) has an oxidation state of 0 on both sides of the equation.
Hydrogen (H) in HCl has an oxidation state of +1, and in H2, it has an oxidation state of 0.
Chlorine (Cl) in HCl has an oxidation state of -1, and in ZnCl2, it has an oxidation state of -1.
From the comparison, we can see that hydrogen is reduced from an oxidation state of +1 to 0. This means that hydrogen is being reduced in the reaction.
On the other hand, zinc is oxidized from an oxidation state of 0 to +2 in ZnCl2. This indicates that zinc is being oxidized in the reaction.
To summarize:
- Hydrogen (H) is reduced.
- Zinc (Zn) is oxidized.