Write procedure of oxidation number change method.
Answers
Answer:
it is quite big but I hope it will help you
Explanation:
Step 1: Assign oxidation numbers to each of the atoms in the equation and write the numbers above the atom.
Step 2: Identify the atoms that are oxidized and those that are reduced. In the above equation, the carbon atom is being oxidized since its oxidation increases from +2 to +4. The iron atom is being reduced since its oxidation number decreases from +3 to 0.
Step 3: Use a line to connect the atoms that are undergoing a change in oxidation number. On the line, write the oxidation-number change.
Walkthrough of connecting atoms that are oxidized or reduced in a redox reaction
The carbon atom’s oxidation number increases by 2, while the iron atom’s oxidation number decreases by 3. As written, the number of electrons lost does not equal the number of electrons gained. In a balanced redox equation, these must be equal. So, the increase in oxidation number of one atom must be made equal to the decrease in oxidation number of the other.
Step 4: Use coefficients to make the total increase in oxidation number equal to the total decrease in oxidation number. In this case, the least common multiple of 2 and 3 is 6. So the oxidation-number increase should be multiplied by 3, while the oxidation-number decrease should be multiplied by 2. The coefficient is also applied to the formulas in the equation. So a 3 is placed in front of the CO and in front of the CO2. A 2 is placed in front of the Fe on the right side of the equation. The Fe2O3 does not require a coefficient because the subscript of 2 after the Fe indicates that there are already two iron atoms.
Walkthrough of balancing the atoms being reduced or oxidized
Step 5: Check the balancing for both atoms and charge. Occasionally, a coefficient may need to be placed in front of a molecular formula that was not involved in the redox process. In the current example, the equation is now balanced.
The general procedure involves the following steps:-
1. Select the atom in oxidising agent whose Oxidation number decreases and indicate the gain of electrons.
2. Select the atom in reducing agent whose oxidation number increases and indicate the loss of electrons.
3. Now cross multiply i.e.multiply Oxidising agent by the number of loss of electrons and reducing agent by number of gain ot electrons.
4. Balance the number ol atoms on both sides whose oxidation numbers change in the reaction.
5. In order to balance oxygen atoms, add HO molecules to the side deficient in oxygen.
6. Then balance the number of H atoms by adding H° ions to the side deficient in hydrogen.