In 1986 an electrical power plant in Taylorsville, Georgia, burned 8,376,726 tons of coal, a national record at that time. (b) If 55% of the SO 2 could be removed by reaction with powdered CaO to form CaSO 3 , how many tons of CaSO 3 would be produced?

First, understand the chemical reaction involved: sulfur dioxide (SO_{2}) reacts with calcium oxide (CaO) to form calcium sulfite (CaSO_{3}). The balanced chemical equation is: SO_{2} + CaO → CaSO_{3}.. Determine the amount of SO_{2} that can be removed. Since 55% of the SO_{2} is removed, calculate the mass of SO_{2} that reacts using the total mass of coal burned. Assume the coal contains a certain percentage of sulfur, which will be converted to SO_{2}.. Calculate the moles of SO_{2} removed using its molar mass. Use the formula: moles = mass (in tons) / molar mass (in g/mol). Convert tons to grams for this calculation.. Using the stoichiometry of the reaction, determine the moles of CaSO_{3} produced. Since the reaction is a 1:1 ratio, the moles of CaSO_{3} produced will be equal to the moles of SO_{2} removed.. Convert the moles of CaSO_{3} to tons using its molar mass. Use the formula: mass (in tons) = moles × molar mass (in g/mol) / conversion factor from grams to tons.

In 1986 an electrical power plant in Taylorsville, Georgia, burned 8,376,726 tons of coal, a national record at that time. (b) If 55% of the SO2 could be removed by reaction with powdered CaO to form CaSO3, how many tons of CaSO3 would be produced?

First, understand the chemical reaction involved: sulfur dioxide (SO_{2}) reacts with calcium oxide (CaO) to form calcium sulfite (CaSO_{3}). The balanced chemical equation is: SO_{2} + CaO → CaSO_{3}. Determine the amount of SO_{2} that can be removed. Since 55% of the SO_{2} is removed, calculate the mass of SO_{2} that reacts using the total mass of coal burned. Assume the coal contains a certain percentage of sulfur, which will be converted to SO_{2}. Calculate the moles of SO_{2} removed using its molar mass. Use the formula: moles = mass (in tons) / molar mass (in g/mol). Convert tons to grams for this calculation. Using the stoichiometry of the reaction, determine the moles of CaSO_{3} produced. Since the reaction is a 1:1 ratio, the moles of CaSO_{3} produced will be equal to the moles of SO_{2} removed. Convert the moles of CaSO_{3} to tons using its molar mass. Use the formula: mass (in tons) = moles × molar mass (in g/mol) / conversion factor from grams to tons.

Ch.18 - Chemistry of the Environment

Brown - Chemistry: The Central Science 14th Edition

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Brown 14th Edition

Ch.18 - Chemistry of the Environment

문제 79b

18장, 문제 79b

In 1986 an electrical power plant in Taylorsville, Georgia, burned 8,376,726 tons of coal, a national record at that time. (b) If 55% of the SO₂ could be removed by reaction with powdered CaO to form CaSO₃, how many tons of CaSO₃ would be produced?

검증된 단계별 안내

First, understand the chemical reaction involved: sulfur dioxide (SO₂) reacts with calcium oxide (CaO) to form calcium sulfite (CaSO₃). The balanced chemical equation is: SO₂ + CaO → CaSO₃.

Determine the amount of SO₂ that can be removed. Since 55% of the SO₂ is removed, calculate the mass of SO₂ that reacts using the total mass of coal burned. Assume the coal contains a certain percentage of sulfur, which will be converted to SO₂.

Calculate the moles of SO₂ removed using its molar mass. Use the formula: moles = mass (in tons) / molar mass (in g/mol). Convert tons to grams for this calculation.

Using the stoichiometry of the reaction, determine the moles of CaSO₃ produced. Since the reaction is a 1:1 ratio, the moles of CaSO₃ produced will be equal to the moles of SO₂ removed.

Convert the moles of CaSO₃ to tons using its molar mass. Use the formula: mass (in tons) = moles × molar mass (in g/mol) / conversion factor from grams to tons.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It involves using balanced chemical equations to determine the proportions of substances consumed and produced. In this case, understanding the stoichiometric relationship between sulfur dioxide (SO2) and calcium oxide (CaO) is essential to calculate the amount of calcium sulfate (CaSO3) formed.

Chemical Reactions

Chemical reactions involve the transformation of reactants into products through breaking and forming chemical bonds. The specific reaction in this scenario is the neutralization of sulfur dioxide with calcium oxide to produce calcium sulfate. Recognizing the type of reaction and the products formed is crucial for determining the quantities involved.

Mass Percent and Yield

Mass percent refers to the percentage of a specific component in a mixture or compound, while yield indicates the amount of product obtained from a reaction compared to the theoretical maximum. In this question, calculating the mass of CaSO3 produced requires understanding the mass percent of SO2 removed and applying it to the total coal burned to find the resultant product mass.