Manganese can be oxidized all the way up to +7, so conceivably
6 K2MnO4 +O3 -> 3 K20 + 6 KMnO4
is possible. However the most stable oxidation state of Manganese is +2 so you would have to 'hit it pretty hard' with a lot of energy to get it all the way up to +7.
The compound name for K2MnO4 is potassium permanganate.
Bromine reacts with ozone through a radical chain mechanism, which ultimately leads to the destruction of ozone molecules. Bromine radicals are released from bromine-containing compounds, reacting with ozone molecules and catalyzing the breakdown of ozone into oxygen molecules. This process contributes to ozone depletion in the atmosphere.
In order to convert KMnO4 to K2MnO4, a reducing agent is typically needed. One common method involves using a reducing agent like a metal, such as zinc or iron, to react with KMnO4 in an acidic medium to produce K2MnO4.
In K2MnO4, the oxidation state of oxygen is -2, and the overall charge of the compound is -1. Given that potassium has a +1 oxidation state, the oxidation state of manganese (Mn) in this compound is +7.
Sulfur dioxide contributes to ozone depletion when it reacts with other chemicals in the atmosphere, forming sulfur trioxide and sulfuric acid. These compounds can then accumulate on ice particles in the stratosphere, leading to the formation of ozone-depleting polar stratospheric clouds. Consequently, sulfur dioxide indirectly impacts the ozone layer by facilitating the destruction of ozone molecules.
Farts, being easily oxidized, do not survive to reach the ozone layer. Ozone will attack them, if released on high pollution advisory days.
The compound name for K2MnO4 is potassium permanganate.
water vapor, oxidized
Bromine reacts with ozone through a radical chain mechanism, which ultimately leads to the destruction of ozone molecules. Bromine radicals are released from bromine-containing compounds, reacting with ozone molecules and catalyzing the breakdown of ozone into oxygen molecules. This process contributes to ozone depletion in the atmosphere.
In order to convert KMnO4 to K2MnO4, a reducing agent is typically needed. One common method involves using a reducing agent like a metal, such as zinc or iron, to react with KMnO4 in an acidic medium to produce K2MnO4.
Treated with ozone As(III) in solution is oxidized to As(V); then arsenic can be precipitated with iron sulfate. This process may be used for deleting arsenic from industrial water wastes.
At low pH value this decomposition takes place: 3 K2MnO4 + 2 H2O → 2 KMnO4 + MnO2 + 4 KOH
Ozone and hydrogen do not react directly, in general. Hydrogen does get oxidized to water vapor, and water vapor does destroy ozone to make hydrogen peroxide. It just takes a couple of intermediate steps.
Equivalent weight of KMnO4 is equal with molar weight of KMnO4. The some is and for K2MnO4, K2MnO4 - e +OH- --------- KMnO4 + KOH In general, Equivalent weight = Molar weight / Number of electrons that take or give one molecule Equivalent weight of KMnO4 = Molar weight of KMnO4 / 1
In K2MnO4, the oxidation state of oxygen is -2, and the overall charge of the compound is -1. Given that potassium has a +1 oxidation state, the oxidation state of manganese (Mn) in this compound is +7.
Everything in chemistry is relative. KMnO3 is a very powerful oxidizing agent and it is more powerful than ozone (O3), so it would not be oxidized by it.
Chlorofluorocarbons (CFCs) and halons are the main chemicals responsible for ozone depletion. They are released from sources like refrigerants, solvents, and fire extinguishers. When these chemicals reach the stratosphere, they break down and release chlorine and bromine atoms that destroy ozone molecules.