Ethylene (CH,CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 100 kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH,CH,) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 60.0 L reaction tank with 46.0 atm of ethane gas and raises the temperature to 400. °C. He believes K=0.30 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of K, and the mass percent of ethylene you calculate may not be what he actually observes. %

Ethylene (CH,CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 100 kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH,CH,) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 60.0 L reaction tank with 46.0 atm of ethane gas and raises the temperature to 400. °C. He believes K=0.30 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of K, and the mass percent of ethylene you calculate may not be what he actually observes. %

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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Question

Ethylene (CH,CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10° kg of polyethylene are made
from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world
demand, so ethane (CH,CH,3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and
hydrogen gas.
Suppose an engineer studying ethane cracking fills a 60.0 L reaction tank with 46.0 atm of ethane gas and raises the temperature to 400. °C. He believes
K,=0.30 at this temperature.
Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits.
Note for advanced students: the engineer may be mistaken about the correct value of K, and the mass percent of ethylene you calculate may not be what he
actually observes.
%
x10

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