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 s(s) + o2(g) → so2(g) how much sulfur (in tons), present in the original materials, would result in that quantity of so2?

Answer 1

Answer: The mass of sulfur produced is $1.305\times 10^{-4}tons$

Explanation:

We are given:

Mass of sulfur dioxide = 26 million tons = $235.872\times 10^{11}g$    (Conversion factor:  $\text{1 million ton}=9.072\times 10^{11}g$ )

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

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$      .....(1)

Given mass of sulfur dioxide = $235.872\times 10^{11}g$

Molar mass of sulfur dioxide = 64 g/mol

Putting values in equation 1, we get:

$\text{Moles of sulfur dioxide}=\frac{235.872\times 10^{11}g}{64g/mol}=3.70\times 10^{11}mol$

For the given chemical equation:

$S(s)+O_2(g)\rightarrow SO_2(g)$

By Stoichiometry of the reaction:

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

So, $3.70\times 10^{11}$ moles of sulfur dioxide will be produced by = $\frac{1}{1}\times 3.70\times 10^{11}=3.70\times 10^{11}$ moles of sulfur.

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

Molar mass of sulfur = 32 g/mol

Moles of sulfur = $3.70\times 10^{11}mol$

Putting values in equation 1, we get:

$3.70\times 10^{11}mol=\frac{\text{Mass of sulfur}}{32g/mol}\\\\\text{Mass of sulfur}=(32g/mol\times 3.70\times 10^{11}mol)=118.4\times 10^{11}g$

Converting this into tons, we use the conversion factor:

1 ton = 907185 grams

So, $118.4\times 10^{11}g\times \frac{1ton}{907185g}=1.305\times 10^{-4}tons$

Hence, the mass of sulfur produced is $1.305\times 10^{-4}tons$

Answer 2

Answer is: quantity of sulfur is 13 tons.

Chemical reaction: S(s) + O₂(g) → SO₂(g).

From chemical reaction: n(S) : n(SO₂) = 1 : 1.

n(S) = n(SO₂); amount of substance.

m(S) ÷ M(S) = m(SO₂) : M(SO₂).

m(S) : 32 g/mol = 26 t : 64 g/mol.

m(S) = (32 g/mol · 26 t) ÷ 64 g/mol.

m(S) = 13 t = 13000 kg; mass of sulfur.