in the equation, KCL+Pb(No3)2+PbCl2. what is reducing and what is being oxidized
To determine what is being reduced and what is being oxidized in the given equation, you need to identify the oxidation numbers of each element. The oxidation number is a positive or negative number assigned to each atom in a compound or ion to indicate its apparent charge.
Let's break down the given equation into its components:
1. KCl: K has an oxidation number of +1, and Cl has an oxidation number of -1.
2. Pb(NO3)2: Pb has an unknown oxidation number, and NO3 has an oxidation number of -1.
3. PbCl2: Pb has an unknown oxidation number, and Cl has an oxidation number of -1.
Now, we need to determine the changes in oxidation numbers for the elements involved to identify which one is reduced and which one is oxidized. Oxidation refers to an increase in the oxidation number, while reduction refers to a decrease.
In this case, we have Pb going from an unknown oxidation number to +2 in PbCl2. Therefore, Pb is being reduced as its oxidation number decreases from an unknown number to +2.
On the other hand, the NO3 ion goes from an oxidation number of -1 in Pb(NO3)2 to an oxidation number of 0 in PbCl2. Since the oxidation number of the N atom goes from +5 to 0, it is being reduced. However, the Pb atom is being oxidized.
To summarize:
- Pb is being reduced.
- NO3 is being reduced.
- Cl remains constant in terms of oxidation number.
Please note that this explanation assumes the reaction is occurring in an aqueous solution and that Pb has an oxidation state of +2 in PbCl2.