i need to balance this redox euation
Mn+2 +H2O2----- MnO2 + H2O
Try this. The Mn was oxidzed, and half the O was reduced.
Mn+2 +2H2O2----- MnO2 + 2H2O
i do not have idea about the answer
I am confused..
To balance the redox equation Mn+2 + H2O2 → MnO2 + H2O, we'll follow these steps:
Step 1: Determine the oxidation states of each element in the equation. Let's assign the oxidation states:
Mn+2 + H2O2 → MnO2 + H2O
Mn: +2 → +4
H: +1 → +1
O: -1 → -1
Step 2: Identify which elements are being oxidized and reduced. In this reaction, the manganese (Mn) is being both oxidized and reduced.
Step 3: Start balancing the equation by balancing the elements that are undergoing oxidation or reduction. In this case, there are two manganese atoms being oxidized:
Mn+2 → MnO2
To balance the manganese atoms, we need to add two hydroxide ions (OH-) to the left-hand side of the equation:
Mn+2 + 2OH- → MnO2
Step 4: Next, balance the oxygen atoms by adding water (H2O) to the right-hand side:
Mn+2 + 2OH- → MnO2 + H2O
Step 5: Balance the hydrogen atoms by adding protons (H+) to the left-hand side:
Mn+2 + 2OH- + 4H+ → MnO2 + H2O
Step 6: Finally, balance the charge by adding electrons (e-) to the appropriate side of the equation. In this case, the charge on the left-hand side is +2, while the charge on the right-hand side is 0. Therefore, we need to add 2 electrons to the left-hand side:
Mn+2 + 2OH- + 4H+ + 2e- → MnO2 + H2O
Now, the equation is balanced with respect to both mass and charge.