ework Due in an Octasulfur(Sg) is the most common allotrope of sulfur and is widely used in the chemical industry, especially in the production of petroleum. While Sg is the main component of elemental sulfur on earth is can also be produced in the laboratory from the reaction of sulfur dioxide with hydrogen sulfide. The balanced chemical equation for this reaction is shown below: 8SO (g) + 16H2S(g) 3S8(s) + 16H,0(g) Consider the reaction of 93.0 grams of SO, with 93.0 grams of H2Sto answer the questions below. Drag and drop options on the right-hand side and submit. For keyboard navigation. SHOW MORE v What is the limiting reagent? H,S What is the excess reagent? 87.1 grams How many grams of Sg can be formed? 131 grams How many grams of excess reagent are left over? 5.77 grams [Fulls 10:38 PM II

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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.