While ethanol (CH, CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized byreacting ethylene (CH₂CH₂) with water vapor at elevated temperatures.A chemical engineer studying this reaction fills a 2.0 L flask with 2.1 atm of ethylene gas and 3.2 atm of water vapor. When the mixturehas come to equilibrium she determines that it contains 0.50 atm of ethylene gas and 1.6 atm of water vapor.The engineer then adds another 1.1 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanolafter equilibrium is reached the second time. Round your answer to 2 significant digits.

Answered: Image /qna-images/answer/efe6cf32-9eb3-4576-94c1-b137ce8c6145.jpg

While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 2.0 L. flask with 2.1 atm of ethylene gas and 3.2 atm of water va has come to equilibrium she determines that it contains 0.50 atm of ethylene gas and 1.6 atm of water vapor. The engineer then adds another 1.1 atm of water, and allows the mixture to come to equilibrium again. Calculate after equilibrium is reached the second time. Round your answer to 2 significant digits.

While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 2.0 L. flask with 2.1 atm of ethylene gas and 3.2 atm of water va has come to equilibrium she determines that it contains 0.50 atm of ethylene gas and 1.6 atm of water vapor. The engineer then adds another 1.1 atm of water, and allows the mixture to come to equilibrium again. Calculate after equilibrium is reached the second time. Round your answer to 2 significant digits.

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...

See similar textbooks

Similar questions

At a certain temperature, 0.302 mol CH, and 0.605 mol H, S are placed in a 1.50 L container. CH,(g) + 2 H, S(g)= CS,(g) + 4 H,(g) At equilibrium, 9.59 g CS, is present. Calculate K.. Ke 8.396 Incorrect
A student ran the following reaction in the laboratory at 479 K: PCI3(g) + Cl₂(g) =PC15(g) When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she found that the equilibrium partial pressure of PCI5 was 1.12 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 200. mL flask with 1.7 atm of ethylene gas and 2.2 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.92 atm of ethylene gas and 1.42 atm of water vapor. olo Ar The engineer then adds another 1.1 atm Of water, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
At a certain temperature, 0.389 mol CH4 and 0.606 mol H₂S are placed in a 3.00 L container. CH₂(g) + 2 H₂S(g) = CS₂(g) + 4H₂(g) At equilibrium, 12.3 g CS₂ is present. Calculate Kc. 2 Вс =
A 10.0 g sample of liquid water is closed in a 1515 mL flask and allowed to reach equilibrium with its vapor at 27ºC. >What is the mass of H2O(g) when equilibrium is established? Data: Pv (H2O, 27ºC) = 26.7 torr.
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S₂(g) + C(s) = CS₂(g) Kc = 9.40 at 900 K How many grams of CS₂ (g) can be prepared by heating 16.3 mol S₂ (g) with excess carbon in a 9.35 L reaction vessel held at 900 K until equilibrium is attained? mass of CS₂ (g): .168 Incorrect g
Consider the following reaction where K, = 9.52×10-2 at 350 K: %3D CH4(g) + CC14(g) 2CH2C1½(g) If the three gases are mixed in a rigid container at 350 K so that the partial pressure of each gas is initially one atm, what will happen? Indicate True (T) or False (F) for each of the following: • 1. A reaction will occur in which CH,Cl2(g) is consumed. v 2. K, will increase. • 3. A reaction will occur in which CH, is consumed. • 4. Q is less than K. v 5. The reaction is at equilibrium. No further reaction will occur.
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 500. mL flask with 2.9 atm of ethylene gas and 1.7 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 2.14 atm of ethylene gas and 0.94 atm of water vapor. The engineer then adds another 0.97 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S₂(g) + C(s) CS₂(g) Kc = 9.40 at 900 K How many grams of CS₂(g) can be prepared by heating 13.4 mol S₂(g) with excess carbon in a 5.65 L reaction vessel held at 900 K until equilibrium is attained? mass of CS₂(g): 6.0 g
Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 125.L tank at 13.°C with 16.mol of nitrogen dioxide gas. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 6.9mol of nitrogen dioxide gas. The engineer then adds another 8.0mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.
A researcher put 0.640 mol PCl3 and 0.768 mol Cl2 into a 2.80 L vessel at a given temperature to produce phosphorus pentachloride, PCI5 : PCI3 (9) + Cl2 (9) =PCl; (g) What will be the composition of this gaseous mixture at equilibrium? K. = 25.6 at the temperature of this experiment. [PCI3] = M [Cl2] M [PCI5] =| M
In a certain experiment 7.50 mile of NH3 was placed in an empty 1.0 liter flask at 900C. After equilibrium was reached, 0.50 mile of N2 was found to be in the flask (along with other gases). Calculate the [NH3] and [H2] at equilibrium and the numerical value of Kc. 2NH3 (g) = N2(g) + 3H2(g)