The hydroperoxide ion, HO2– (aq), reacts with permanganate ion, MnO4– (aq) to produce MnO2 (s) and oxygen gas. Balance the equation for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution.
hkgv
To balance the equation for the oxidation of hydroperoxide ion to oxygen gas by permanganate ion in a basic solution, follow these steps:
Step 1: Write the unbalanced equation.
HO2– (aq) + MnO4– (aq) → MnO2 (s) + O2(g)
Step 2: Balance the oxygen atoms by adding water (H2O) molecules to the appropriate side.
HO2– (aq) + MnO4– (aq) → MnO2 (s) + O2(g) + H2O(l)
Step 3: Balance the hydrogen atoms by adding hydrogen ions (H+) to the appropriate side.
HO2– (aq) + MnO4– (aq) + H2O(l) → MnO2 (s) + O2(g) + H2O(l)
Step 4: Balance the charge by adding electrons (e–).
HO2– (aq) + MnO4– (aq) + H2O(l) → MnO2 (s) + O2(g) + H2O(l) + e–
Step 5: Determine the number of electrons needed for the reaction by comparing the oxidation states of the elements involved.
The oxidation state of oxygen in HO2– is -1, while the oxidation state of oxygen in O2 is 0. Hence, each oxygen atom gains 2 electrons.
The oxidation state of manganese in MnO4– is +7, while the oxidation state of manganese in MnO2 is +4. Hence, each manganese atom loses 3 electrons.
Step 6: Multiply the half-reactions by appropriate numbers to balance the electrons.
2HO2– (aq) + 2MnO4– (aq) + 4H2O(l) → 2MnO2 (s) + 2O2(g) + 4H2O(l) + 4e–
Step 7: Combine the half-reactions and cancel out the common substances on both sides.
2HO2– (aq) + 2MnO4– (aq) + 4H2O(l) → 2MnO2 (s) + 2O2(g) + 4H2O(l) + 4e–
Cancel out the 4H2O(l) on both sides.
2HO2– (aq) + 2MnO4– (aq) → 2MnO2 (s) + 2O2(g) + 4e–
Step 8: Combine the electron transfer and simplify.
2HO2– (aq) + 2MnO4– (aq) → 2MnO2 (s) + O2(g) + 2H2O(l)
The balanced equation for the oxidation of hydroperoxide ion to oxygen gas by permanganate ion in a basic solution is:
2HO2– (aq) + 2MnO4– (aq) → 2MnO2 (s) + O2(g) + 2H2O(l)
To balance the equation for the oxidation of hydroperoxide ion (HO2–) to O2(g) by permanganate ion (MnO4–) in a basic solution, you need to follow these steps:
Step 1: Write the unbalanced chemical equation.
HO2–(aq) + MnO4–(aq) → MnO2(s) + O2(g)
Step 2: Balance the elements other than oxygen and hydrogen.
The equation currently has one manganese (Mn) atom, one oxygen (O) atom, and two hydrogen (H) atoms on each side. Balance them by adding the appropriate coefficients in front of the compounds.
2 HO2–(aq) + MnO4–(aq) → MnO2(s) + O2(g)
Step 3: Balance the oxygen atoms.
On the left side, we have 2 oxygen atoms from the hydroperoxide ion (2 HO2–), and on the right side, we have 2 oxygen atoms from the manganese dioxide (MnO2). Therefore, the oxygen atoms are already balanced.
Step 4: Balance the hydrogen atoms.
On the left side, we have 4 hydrogen atoms from the two hydroperoxide ions (2 HO2–). On the right side, we have 2 hydrogen atoms from water (H2O), which is not present in the unbalanced equation. To balance the hydrogen atoms, add 4 H2O to the left side.
2 HO2–(aq) + MnO4–(aq) + 4 H2O → MnO2(s) + O2(g)
Step 5: Balance the charge.
On the left side, we have -2 charge from each hydroperoxide ion (2 HO2–) and -1 charge from the permanganate ion (MnO4–). On the right side, we have 0 charge from manganese dioxide (MnO2), and oxygen gas (O2) has no charge. To balance the charge, add 8 OH– ions to the left side.
2 HO2–(aq) + MnO4–(aq) + 4 H2O + 8 OH–(aq) → MnO2(s) + O2(g)
Step 6: Verify and simplify the equation.
Double-check that all elements and charges are balanced. In the simplified equation, it becomes:
2 HO2–(aq) + MnO4–(aq) + 4 H2O + 8 OH–(aq) → MnO2(s) + O2(g)
Now the equation is balanced for the oxidation of hydroperoxide ion to O2(g) by permanganate ion in a basic solution.