Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this synthesis, called the Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water. Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 442. liters per second of dioxygen are consumed when the reaction is run at 247. °C and the dioxygen is supplied at 0.74 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. 0 55 x10 G
Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this synthesis, called the Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water. Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 442. liters per second of dioxygen are consumed when the reaction is run at 247. °C and the dioxygen is supplied at 0.74 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. 0 55 x10 G
General Chemistry - Standalone book (MindTap Course List)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.158QP: An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the...
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Transcribed Image Text:Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this
synthesis, called the Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water.
Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 442. liters per second of dioxygen are consumed when the reaction is run
at 247. °C and the dioxygen is supplied at 0.74 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second.
Round your answer to 2 significant digits.
0
55
x10
G
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