7) Hydrogen Sulfide is an impurity in natural gas that must be removed. One common removal method is called the Claus process, which relies on the reaction: 8 H2S(g) + 4O2(g) S8(l) + 8 H2O Under optimal conditions the Claus process gives 98% yield of S8 from H2S. If you started with 30.0 grams of H2S and 50.0 grams of O2, how many grams of S8 would be produced, assuming 98.0% yield?
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
7) Hydrogen Sulfide is an impurity in natural gas that must be removed. One common removal
method is called the Claus process, which relies on the reaction:
8 H2S(g) + 4O2(g) S8(l) + 8 H2O
Under optimal conditions the Claus process gives 98% yield of S8 from H2S. If you started with 30.0
grams of H2S and 50.0 grams of O2, how many grams of S8 would be produced, assuming 98.0%
yield?
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Why do you multipy the # of H2S mols by 4, when 4 corresponds to the reactory amount of O2?
The logic there is somewhat confusing to me.
I understand how/why you found out the mols of the equation but dividing the sample's MM by the equation confuses me.
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