The annual production of sulfur dioxide from burning coal and fossil fuels, auto exhaust, and other sources is about 26 million tons. the equation for the reaction is s(s) + o2(g) → so2(g) how much sulfur (in tons), present in the original materials, would result in that quantity of so2?

The mass of sulfur produced is

Explanation:

We are given:

Mass of sulfur dioxide = 26 million tons =    (Conversion factor:   )

To calculate the number of moles, we use the equation:

     .....(1)

Given mass of sulfur dioxide =

Molar mass of sulfur dioxide = 64 g/mol

Putting values in equation 1, we get:

For the given chemical equation:

By Stoichiometry of the reaction:

1 mole of sulfur dioxide is produced by 1 mole of Sulfur.

So, moles of sulfur dioxide will be produced by = moles of sulfur.

Calculating the mass of sulfur by using equation 1, we get:

Molar mass of sulfur = 32 g/mol

Moles of sulfur =

Putting values in equation 1, we get:

Converting this into tons, we use the conversion factor:

1 ton = 907185 grams

So,

Hence, the mass of sulfur produced is

lab safety rules

explanation: