The equation 5KMnO4 + 3H2C2O4 -> 5K2C2O4 + 3MnSO4 + 4H2O + 5O2

Detailed information:

• The given equation is an equation for a redox reaction. KMnO₄ is a strong oxidizing agent, capable of oxidizing H₂C₂O₄ (oxalic acid) to K₂C₂O₄ (Potassium oxalate). During this process, KMnO₄ is reduced to MnSO₄.
• The molar amount of the reacting substances is represented by the coefficients in the chemical equation: 5 moles of KMnO₄ react with 3 moles of H₂C₂O₄ to produce 5 moles of K₂C₂O₄, 3 moles of MnSO₄, 4 moles of H₂O and 5 moles of O₂.

Reaction conditions:

• The reaction typically occurs in an acidic environment. In other words, a condition for the reaction is the presence of H+ ions.
• Meanwhile, temperature also influences the reaction rate. Increasing the temperature will increase the reaction rate.

Reaction process:

• Oxidation process: 2H₂C₂O₄ -> 2K₂C₂O₄ + CO₂ + H₂O ->
• Reduction process: 5KMnO₄ + H₂O -> 3MnSO₄ + 5K₂C₂O₄ + 5O₂

Observed phenomena:

• The KMnO₄ solution, which is purple-red in color, gradually turns colorless as MnSO₄ is colorless.
• O₂ gas is released.
• During the reaction, if there are other strong reducing agents present, KMnO₄ may be completely reduced to Mn₂+, causing the solution to turn light pink due to the presence of Mn₂+ ions.