OKINETICS AND EQUILIBRIUM Calculating the reaction rate of one reactant from that of another 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 203. liters per second of dioxygen are consumed when the reaction is run at 262. °C and the dioxygen is supplied at 0.98 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. O - 15 X do

OKINETICS AND EQUILIBRIUM Calculating the reaction rate of one reactant from that of another 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 203. liters per second of dioxygen are consumed when the reaction is run at 262. °C and the dioxygen is supplied at 0.98 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. O - 15 X do

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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Two chemicals A and B are combined to form a chemical C. The rate, or velocity, of the reaction is proportional to the product of the instantaneous amounts of A and B not converted to chemical C. Initially, there are 40 grams of A and 50 grams of B, and for each gram of B, 2 grams of A is used. It is observed that 10 grams of C is formed in 8 minutes. How much (in grams) is formed in 16 minutes? (Round your answer to one decimal place.) grams What is the limiting amount (in grams) of C after a long time? grams How much (in grams) of chemicals A and B remains after a long time? A B grams grams
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Calculating the reaction rate of one reactant from that of another Nitric acid is a key industrial chemical, largely used to make fertilizers and explosives. The first step in its synthesis is the oxidation of ammonia. In this reaction, gaseous ammonia reacts with dioxygen gas to produce nitrogen monoxide gas and water. alo Suppose a chemical engineer studying a new catalyst for the oxidation of ammonia reaction finds that 514. liters per second of dioxygen are consumed when the reaction is run at 213. °c and the dioxygen is supplied at 0.64 atm. Calculate the rate at which nitrogen monoxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. Ar kg x10 S ||
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Questions 7 through 11 refer to the information and diagram below. 2 NO2(g) > N204(g) NO2(8) reacts to form N20a(g) according to the equation above. A pure sample of NO2(g) is placed into a rigid, evacuated 0.500 L container. The initial pressure of the NO2(g) is 960 torr. The temperature is held constant until the NO2(g) reaches equilibrium with its product. The figure below shows how the pressure of the system changes while reaching equilibrium. Pressure (torr) 960 760 Time 8. The pressure vs. time curve can be used to evaluate (A) only the value of Q. (B) only the equilibrium constant from the horizontal part. (C) only the kinetics of the reaction from the decreasing part. (D) the kinetics of the reaction from the decreasing part and the equilibrium constant from the horizontal part.
O KINETICS AND EQUILIBRIUM Calculating the reaction rate of one reactant from that of another Esther v The reform reaction between steam and gaseous methane (CH) produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. Synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen. Suppose a chemical engineer studying a new catalyst for the reform reaction finds that 204. liters per second of methane are consumed when the reaction is run at 240. °C and the methane is supplied at 0.33 atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. do kg Explanation Check Privacy Accessibility O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use 642 4 MacBook Air 4) F10 888 F7 F5 F4 esc F2 F3 FI %3D %23 $ 6. 8 3 4. 1 Y R Q W
Which of the following reactions, carried out in a closed container, will result in a reduced total pressure? a. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) b. 2N2O(g) → 2N2(g) + O2(g) c. 2HI(g) → H2(g) + I2(g) d. 2H2(g) + O2(g) → 2H2O(l) e. None of these reactions will result in a pressure reduction.
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