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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The reaction rate of a chemical reaction will increase as a result of changes made to the system, as long as those changes increase what factor? O Amount of empty space between reactants O Number of collisions between reactants O Electrical charge of the reactants O Atomic mass of the reactants
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.
A flask is charged with 0.140 mol of A and allowed to react to form B according to the following hypothetical gas-phase reaction. A(g) → B(g) The following data are collected. Os 0 40 S 0.072 80 s 0.025 120 s 0.014 (a) Calculate the number of moles of B at each time in the table. 160 s 0.013 0 - 40 s 0.0018 40 - 80 s 0.000625 80 - 120 s 0.00035 120 - 160 mol/s 0.000325 times (s) mol mol x mol x mol moles of A X mol mol/s mol/s 0 (b) Calculate the average rate of disappearance of A for each 40 s interval, in units of mol/s. mol/s 40 mol/s 80 120 0.140 0.068 0.043 0.029 160 0.016
How does a common intermediate couple two chemicalreactions?
The reform reaction between steam and gaseous methane ( CH4 ) 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 526. liters per second of methane are consumed when the reaction is run at 186.°C and 0.36atm . 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.
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6) Complete the following ICE table. All of the reactants and products for this reaction are gases, and the temperature and volume are constant during the reaction. 7 F2 2 CF4 329.5 89.1 Initial pressure (torr): Change (torr): Ending pressure (torr): C₂H6 127.3 + + 6 HF 0
If a sample of nitrogen gas in a sealed container of fixed volume is heated from 25°C to 150°C, the Value of following quantities will remain constant? O the average speed of the molecules O the density of the nitrogen O the average intensity of a molecular collision with the walls of the container the average kinetic energy of the molecules O the pressure of the gas
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Coal gasification produces an easily-transportable, clean-burning combination of carbon monoxide and hydrogen from coal by reacting it with steam, like this: C(s) + H₂O(g) → CO(g) +H₂(g) Suppose an engineer decides to study the rate of this reaction. He prepares four reaction vessels with 95.1 g of solid carbon and 12.3 g of steam each. The volume and temperature of each vessel is shown in the table below. Arrange the reaction vessels in decreasing order of initial rate of reaction. In other words, select a "1" next to the vessel in which the engineer can reasonably expect the initial rate of reaction to be highest, a "2" next to the vessel in which the initial rate of reaction would be next highest, and so on. vessel volume temperature A B C D 4.0 L 2.0 L 4.0 L 2.0 L 300, "C 310, "C 310 °C 330. "C X initial rate of reaction P ? ? ? G v V