Question

Составить электронный баланс, указать окислитель и восстановитель, процессы окисления и восстановления 1. P2O3+O2--->P2O5 2.Fe+H2SO4--->FeSO4+H2 3.Zn+FeSO4--->ZnSO4+Fe

Answer 1

+3 -2         0       +5 -2
P2O3  +  O2  → P2O5
+3           +5
P - 2e →   P      процесс окисления, восстановитель
0                   -2
O2 +2* 2e →2O  процесс восстановления, окислитель
 0    +1 +6 -2     +2+6-2     0
Fe + H2SO4 → FeSO4 + H2
0              +2
Fe - 2e →Fe  процесс окисления, восстановитель
+1                0
2Н  + 2*1е →Н2 процесс восстановления, окислитель
  0     +2+6-2       +2+6-2     0
Zn +   FeSO4 → ZnSO4 + Fe
 0           +2
Zn -2e→Zn   процесс окисления, восстановитель
+2             0
Fe + 2e →Fe процесс восстановления, окислитель

Answer 2

Electron Balancing and Redox Reactions

To balance the given chemical equations and identify the oxidizing and reducing agents, we need to follow a few steps. Let's go through each equation one by one:

1. P2O3 + O2 → P2O5

To balance this equation, we need to make sure that the number of atoms of each element is the same on both sides. Let's start by balancing the phosphorus (P) atoms:

Step 1: There are 2 phosphorus (P) atoms on the left side and 2 on the right side, so phosphorus is already balanced.

Step 2: Now, let's balance the oxygen (O) atoms. There are 3 oxygen (O) atoms in P2O3 and 5 oxygen (O) atoms in P2O5. To balance the oxygen atoms, we need to add 2 more oxygen (O) molecules (O2) on the left side:

P2O3 + 2O2 → P2O5

Now, the equation is balanced.

To identify the oxidizing and reducing agents, we need to determine the change in oxidation states of the elements involved in the reaction. In this case, the oxidation state of phosphorus changes from +3 in P2O3 to +5 in P2O5. Therefore, phosphorus is being oxidized and oxygen is being reduced.

2. Fe + H2SO4 → FeSO4 + H2

Let's balance this equation:

Step 1: There is 1 iron (Fe) atom on both sides, so iron is already balanced.

Step 2: Now, let's balance the hydrogen (H) atoms. There are 2 hydrogen (H) atoms in H2SO4 and 2 hydrogen (H) atoms in H2. The hydrogen (H) atoms are already balanced.

Step 3: Next, let's balance the sulfur (S) and oxygen (O) atoms. There is 1 sulfur (S) atom on both sides, so sulfur is already balanced. However, there are 4 oxygen (O) atoms in H2SO4 and only 1 oxygen (O) atom in FeSO4. To balance the oxygen atoms, we need to add 3 more oxygen (O) molecules (O2) on the left side:

Fe + H2SO4 + 3O2 → FeSO4 + H2

Now, the equation is balanced.

To identify the oxidizing and reducing agents, we need to determine the change in oxidation states of the elements involved in the reaction. In this case, the oxidation state of iron changes from 0 in Fe to +2 in FeSO4. Therefore, iron is being oxidized and hydrogen is being reduced.

3. Zn + FeSO4 → ZnSO4 + Fe

Let's balance this equation:

Step 1: There is 1 zinc (Zn) atom on both sides, so zinc is already balanced.

Step 2: Now, let's balance the sulfur (S) and oxygen (O) atoms. There is 1 sulfur (S) atom on both sides, so sulfur is already balanced. However, there are 4 oxygen (O) atoms in FeSO4 and only 4 oxygen (O) atoms in ZnSO4. The oxygen (O) atoms are already balanced.

Step 3: Next, let's balance the iron (Fe) atoms. There is 1 iron (Fe) atom on both sides, so iron is already balanced.

To identify the oxidizing and reducing agents, we need to determine the change in oxidation states of the elements involved in the reaction. In this case, the oxidation state of zinc changes from 0 in Zn to +2 in ZnSO4. Therefore, zinc is being oxidized and iron is being reduced.

In summary:

1. P2O3 + O2 → P2O5 - Oxidizing agent