Final answer:
The question pertains to a chemical reaction involving potassium permanganate and chlorine, but the reference information provided does not give a specific reaction between these chemicals. Instead, it details other reactions and properties of potassium permanganate, including its oxidation state of manganese (+7) and molarity calculations.
Step-by-step explanation:
The student's question involves the reaction between potassium permanganate and chlorine, which are both strong oxidizing agents. However, based on the reference information provided, we are not given a specific reaction between these two chemicals, but instead, several other reactions involving potassium dichromate and potassium permanganate with different chemicals are described. For example, in the case of potassium dichromate, the balanced equation provided is 8 H¯ + Cr₂O²/¯¯ +3 CH₂ CH₂OH → 3 CH₂CHO+2 Cr³+ +7H₂O, and for potassium permanganate with bromide, the reaction products are solid manganese(IV) oxide and aqueous bromate ion, BrO3. However, no direct reaction equations with chlorine are offered.
To address the oxidation state of manganese in potassium permanganate (KMnO4), manganese has an oxidation number of +7, as indicated by the equation [Ar] 4s03d⁰. This state asserts that there are no electrons in the 4s and 3d orbitals of the manganese atom in potassium permanganate. In terms of molarity calculation, dissolving 119 g of potassium permanganate into water to make a 3.00 L solution results in a molarity of 0.250 M.