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 551. liters per second of dioxygen are consumed when the reaction is run at 216. C and the dioxygen is supplied at 0.33 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. Explanation Check 2022 M LLC A yh erd f I y Ce 112 Type here to search 64 A hp E R G K z × | c | B 2|-

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 551. liters per second of dioxygen are consumed when the reaction is run at 216. C and the dioxygen is supplied at 0.33 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. Explanation Check 2022 M LLC A yh erd f I y Ce 112 Type here to search 64 A hp E R G K z × | c | B 2|-

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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 592. liters per second of dioxygen are consumed when the reaction is run at 195. °℃ and the dioxygen is supplied at 0.48 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits.
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Ammonia is among the top ten synthesized compounds. Its many uses include the manufacture of ammonium nitrate and other fertilizers. Ammonia decomposes at high temperatures. In an experiment to explore this behavior, 2.00 moles of gaseous NH3 are sealed in a rigid 1-liter vessel. The vessel is heated at 800 K and some of the NH3 decomposes in the following reaction: 2NH3(g) <--> N2(g)+3H2(g) The system eventually reaches equilibrium and is found to contain 1.74 mole of NH3. What is the value of KC for the decomposition reaction at 800K? What is the value of KP for the decomposition reaction at 800 K?
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How many grams of iron are needed to completely consume 36.4 L of chlorine gas according to the following reaction at 25 °C and 1 atm?iron ( s ) + chlorine ( g ) iron(III) chloride ( s )
For many purposes we can treat methane (CH) as an ideal gas at temperatures above its boiling point of -161. °C. Suppose the temperature of a sample of methane gas is raised from -24.0 °C to 18.0 °C, and at the same time the pressure is changed. If the initial pressure was 6.2 atm and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits. | atm
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Hydrogen gas can be formed by the reaction of methane with water according to the following reaction: CH4(g) + H2O(g) --> CO(g) +3H2(g) In a particular sample, 25.5 L of methane gas (measured at 0.963 atm and 298 K) is mixed with 22.8 L of water vapor (measured at 0.924 atm and 398 K). The reaction generates 26.2 L of di-hydrogen gas at STP. What is the percent yield of the reaction??