Balance using oxidation Number Methode
A. MnO4- + C2H4 + H20 --> MnO2 + OH- + C2H6
B. ClO- --> Cl- +
To balance a chemical equation using the oxidation number method, follow these steps:
1. Assign oxidation numbers to all the atoms in the equation.
2. Identify the atoms that undergo oxidation or reduction.
3. Determine the change in oxidation number for each atom that undergoes a change.
4. Balance the atoms that undergo oxidation and reduction by adjusting the coefficients of the compounds involved.
Now let's apply this method to balance the given equations:
A. MnO4- + C2H4 + H2O --> MnO2 + OH- + C2H6
1. Assign oxidation numbers:
Mn: +7 (since oxygen has an oxidation number of -2 and there are 4 oxygen atoms with a total charge of -8, the chromium must have a charge of +7)
C: -3 (since hydrogen has an oxidation number of +1, and there are 4 hydrogen atoms with a total charge of +4, the carbon must have a charge of -3)
H: +1 (the most common oxidation number for hydrogen is +1)
O: -2 (the most common oxidation number for oxygen is -2)
2. Identify the atoms that undergo oxidation or reduction:
Mn goes from +7 to +4 (reduction)
C goes from -3 to -2 (oxidation)
3. Determine the change in oxidation number:
Mn: Change of -3
C: Change of +1
4. Now, balance the atoms:
MnO4- + 2C2H4 + 2H2O --> MnO2 + 2OH- + 2C2H6
B. ClO- --> Cl-
1. Assign oxidation numbers:
Cl: +1 (since oxygen has an oxidation number of -2 and there is only one oxygen atom with a total charge of -2, the chlorine must have a charge of +1)
2. Identify the atom that undergoes oxidation or reduction:
Cl goes from +1 to -1 (reduction)
3. Determine the change in oxidation number:
Cl: Change of -2
4. Now, balance the atoms:
2ClO- --> 2Cl-