If natural gas contains significant amounts of sulfur as H2 S, it is called sour natural gas. Fo

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If natural gas contains significant amounts of sulfur as H2...

If natural gas contains significant amounts of sulfur as $\mathrm{H}_{2} \mathrm{S}$, it is called sour natural gas. For the gas to be commercially useful as a fuel, the $\mathrm{H}_{2} \mathrm{S}$ must be removed. Once it is separated from the natural gas, it is reacted with oxygen in two different processes to yield either elemental sulfur (S $_{8}$ ), a commercial material that can be sold, or sulfur dioxide $\left(\mathrm{SO}_{2}\right) .$ This sulfur dioxide product can be reacted with more $\mathrm{H}_{2} \mathrm{S}$ to make additional elemental sulfur. Balance the following reactions that describe the production of elemental sulfur. a. $\mathrm{H}_{2} \mathrm{S}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{S}_{8}(s)+\mathrm{H}_{2} \mathrm{O}(g)$. b. $\mathrm{H}_{2} \mathrm{S}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$. $^{*} \mathrm{c} . \mathrm{H}_{2} \mathrm{S}(g)+\mathrm{SO}_{2}(g) \rightarrow \mathrm{S}_{8}(s)+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$.

If natural gas contains significant amounts of sulfur as $\mathrm{H}_{2} \mathrm{S}$, it is called sour natural gas. For the gas to be commercially useful as a fuel, the $\mathrm{H}_{2} \mathrm{S}$ must be removed. Once it is separated from the natural gas, it is reacted with oxygen in two different processes to yield either elemental sulfur (S $_{8}$ ), a commercial material that can be sold, or sulfur dioxide $\left(\mathrm{SO}_{2}\right) .$ This sulfur dioxide product can be reacted with more $\mathrm{H}_{2} \mathrm{S}$ to make additional elemental sulfur. Balance the following reactions that describe the production of elemental sulfur.
a. $\mathrm{H}_{2} \mathrm{S}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{S}_{8}(s)+\mathrm{H}_{2} \mathrm{O}(g)$.
b. $\mathrm{H}_{2} \mathrm{S}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{SO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)$.
$^{*} \mathrm{c} . \mathrm{H}_{2} \mathrm{S}(g)+\mathrm{SO}_{2}(g) \rightarrow \mathrm{S}_{8}(s)+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$.

Key Concepts

Industrial Gas Processing

Industrial gas processing refers to the series of chemical reactions and separation techniques used to treat raw natural gas and remove contaminants to yield commercially valuable products. It involves applied chemical principles, such as reaction balancing and stoichiometry, to efficiently convert undesirable components into useful substances.

Redox Reactions

Redox (reduction-oxidation) reactions are processes that involve the transfer of electrons between species, resulting in changes in their oxidation states. Understanding redox reactions is crucial when dealing with reactions that involve the transformation of sulfur compounds, as it requires identifying which species are oxidized and which are reduced.

Balancing Chemical Equations

Balancing chemical equations is the systematic process of assigning coefficients to the reactants and products in a chemical reaction so that the number of atoms for each element is conserved. This practice is fundamental in ensuring that chemical reactions obey the law of conservation of mass.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It is based on the law of conservation of mass, which ensures that the number of atoms of each element is the same on both sides of a balanced equation. This concept is essential for calculating amounts of substances needed or produced in a reaction.

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