Sulfur dioxide, SO2, forms in the combustion of the sulfur found in fossil fuels such as coal. In the air, SO2 forms SO3, which dissolves in water to form sulfuric acid. Thus SO2 is a major contributor to acid rain as well as a strong eye and lung irritant. The 1990 amendments to the Clean Air Act of 1967 call for a reduction in sulfur dioxide released from power plants to 10 million tons per year. This is about one-half the emission measured in 1990. The US atmospheric standard for SO2 is 0.35 mg/m3, which would yield a pressure due to sulfur dioxide of 0.013 Pa at 17 °C. To what volume in m3 must 1.0 × 107 tons of SO2 expand in order to yield a pressure of 0.013 Pa at 17 °C? (There are 2000 lb per ton.)
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.
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Sulfur dioxide, SO2, forms in the combustion of the sulfur found in fossil fuels such as coal. In the air, SO2 forms SO3, which dissolves in water to form sulfuric acid. Thus SO2 is a major contributor to acid rain as well as a strong eye and lung irritant. The 1990 amendments to the Clean Air Act of 1967 call for a reduction in sulfur dioxide released from power plants to 10 million tons per year. This is about one-half the emission measured in 1990. The US atmospheric standard for SO2 is 0.35 mg/m3, which would yield a pressure due to sulfur dioxide of 0.013 Pa at 17 °C. To what volume in m3 must 1.0 × 107 tons of SO2 expand in order to yield a pressure of 0.013 Pa at 17 °C? (There are 2000 lb per ton.)
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