My question actually is how much would it take to oxidize the sulfur, not how much to get a 1:1 ratio.
The amount it takes to decompose the Hydrogen Sulfide is equal to the amount of Hydrogen Sulfide. That is how the 1:1 ratio is arrived at.
Your question was:
"Having well water with 10 ppm of sulfur, how much 35% peroxide do I have to add per 100 gallon to oxidize the sulfur?"
The first thing that must be done is analyze the chemistry.
Each molecule of H
2S requires one molecule of H
2O
2 to decompose it.
The atomic weight of sulfur is 32, oxygen 16, and hydrogen 1. Therefore, the molecular weight of H
2S is 34 and the molecular weight of H
2O
2 is 34. Since they are the same, the weight ratio is 1:1.
So to figure out much H
2O
2 you need to neutralize 10 mg/L of H
2S in 100 gallons of water using 35% H
2O
2 you must figure out how much H
2S is in the water and use an EQUAL AMOUNT (1:1 ratio) of H
2O
2. Then you must account for the fact that the H
2O
2 is only 35%.
The answer is that you need about 2.2 teaspoons.