Potassium permanganate and oxalic acid

[force]

Does anyone happen to have the rate law for potassium permanganate reacting with oxalic acid ?

I tried searching google with no avail

 

[Borek]

No idea about details, but I recall the reaction is being catalyzed by Mn²⁺, thus it is slow at the beginning, but then gains speed.

 

[Blueshift5]

I can provide some insights on the reaction between potassium permanganate and oxalic acid. This reaction is a redox reaction, where potassium permanganate acts as an oxidizing agent and oxalic acid acts as a reducing agent. The overall reaction equation is:

2KMnO4 + 5H2C2O4 → 2MnC2O4 + 10CO2 + 2K+ + 8H2O

The rate law for this reaction can be determined experimentally by varying the concentrations of both reactants and measuring the rate of the reaction. The general rate law for a redox reaction is:

Rate = k[MnO4-]a [C2O42-]b

where k is the rate constant, [MnO4-] is the concentration of potassium permanganate, [C2O42-] is the concentration of oxalic acid, and a and b are the reaction orders for each reactant, respectively.

The specific values for a and b can only be determined through experimentation. However, based on previous studies, the reaction is known to be first-order with respect to both potassium permanganate and oxalic acid. This means that the rate of the reaction is directly proportional to the concentration of each reactant.

In summary, the rate law for the reaction between potassium permanganate and oxalic acid is likely to be:

Rate = k[MnO4-] [C2O42-]

I hope this helps answer your question. However, it is always recommended to verify the rate law through experimental data.