In the reaction ZnO+2HCl=ZnCl2+H2O what is oxidized and what is reduced?

emmmmm.... are you sure

In the reaction ZnO + 2HCl = ZnCl2 + H2O, zinc oxide (ZnO) is reduced and hydrogen chloride (HCl) is oxidized.

To determine what is oxidized and what is reduced, we need to look at the changes in oxidation numbers of the elements involved in the reaction.

In the reaction, zinc (Zn) in ZnO goes from an oxidation state of +2 to 0 in ZnCl2. This indicates that Zn is gaining electrons and therefore being reduced.

On the other hand, chlorine (Cl) in HCl goes from an oxidation state of -1 to 0 in ZnCl2. This indicates that Cl is losing electrons and therefore being oxidized.

So, zinc oxide (ZnO) is reduced and hydrogen chloride (HCl) is oxidized in the given reaction.

To determine what is oxidized and what is reduced in a chemical reaction, we need to examine the oxidation states of each element involved.

Oxidation refers to an increase in oxidation state (loss of electrons), while reduction refers to a decrease in oxidation state (gain of electrons).

Let's analyze the oxidation states of the elements in the given reaction:
ZnO + 2HCl = ZnCl2 + H2O

The oxidation state of oxygen (O) is typically -2 in compounds. Therefore, in ZnO, the oxidation state of oxygen is -2.

Hydrogen (H) usually has an oxidation state of +1 in compounds, with a few exceptions. In HCl, hydrogen is bonded to chlorine (Cl), which has an oxidation state of -1. Since the overall charge of a compound is 0, the oxidation state of hydrogen in HCl is +1.

Now let's determine the oxidation state of zinc (Zn) in ZnO. Since ZnO is a stable compound, oxygen has an oxidation state of -2, as mentioned earlier. Therefore, the oxidation state of Zn in ZnO must be +2 in order for the overall charge to be 0.

In the product ZnCl2, chlorine has an oxidation state of -1, and there are two chlorine atoms present. Thus, the oxidation state of Zn in ZnCl2 must be +2 (2 x -1 = -2) to balance the overall charge.

Finally, in H2O, we know that oxygen has an oxidation state of -2. To balance the overall charge of 0, hydrogen should have an oxidation state of +1.

By comparing the oxidation states before and after the reaction, we can determine what is oxidized and what is reduced:
Zn is oxidized from an oxidation state of +2 in ZnO to +2 in ZnCl2 (no change in oxidation state).
H is reduced from an oxidation state of +1 in HCl to +1 in H2O (no change in oxidation state).

In summary, in the reaction ZnO + 2HCl = ZnCl2 + H2O, zinc (Zn) is oxidized, and hydrogen (H) is reduced.

Oxidation is the loss of electrons. Reduction is the gain of electrons.

Zn is +2 on the left and +2 on the right. H is +1 on the left and +1 on the right. O is -2 on the left and -2 on the right. Cl is -1 on the left and -1 on the right. Anything change? nope. So nothing is oxidized and nothing is reduced.