# The original sulfur quantity (tons) for 26M tons SO?

Chapter 3, Problem 3.69

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QUESTION:

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

$$\mathrm{S}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g)$$

How much sulfur (in tons), present in the original materials, would result in that quantity of $$\mathrm{SO}_{2}$$?

##### The original sulfur quantity (tons) for 26M tons SO?

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Explore the environmental impact of sulfur dioxide production, revealing how 26 million tons of this compound conceal 13 million tons of sulfur. It delves into the chemistry of this transformation, converting atomic and molecular masses, providing valuable insights into emissions from activities like burning coal and auto exhaust."

QUESTION:

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

$$\mathrm{S}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g)$$

How much sulfur (in tons), present in the original materials, would result in that quantity of $$\mathrm{SO}_{2}$$?

Step 1 of 2

Here we have to calculate the amount of sulphur in tons present in $$\mathrm{SO} 2$$.

The given combustion reaction is, $$\mathrm{S}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{SO}_{2}(\mathrm{~g})$$

The annual production of $$\mathrm{SO}_{2}=26$$ million tons $$=26 \times 10^{7}$$ tons

It is known that atomic mass of $$\mathrm{S}=32.07$$

Molecular mass of $$\mathrm{SO}_{2}=64.07 \mathrm{~g} / \mathrm{mol}$$