Most of the sulfur used In the United States Is chemlcally 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 dloxygen gas to produce gaseous sulfur dloxide and water. Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 474. liters per second of dioxygen are consumed when the reaction is run at 155. °C and the dioxygen Is supplied at 0.41 atm. Calculate the rate at which sulfur dloxide Is being produced. Glve your answer In killograms per second. Be sure your answer has the correct number of significant digits. kg

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