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 25.0 L tank with 6.9 mol of ethylene gas and 11. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 1.5 mol of ethylene gas and 5.6 mol of water vapor. The engineer then adds another 2.8 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. I mol Ox10

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 25.0 L tank with 6.9 mol of ethylene gas and 11. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 1.5 mol of ethylene gas and 5.6 mol of water vapor. The engineer then adds another 2.8 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. I mol Ox10

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

Related questions

Q: ulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Exactly 1.00 mol ClF3 is placed in an empty 1.00-L container (without any products initially) and…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

Q: Suppose a 500. mL flask is filled with 2.0 mol of N, and 0.80 mol of NO. This reaction becomes…

A: To fill the missing part in the table , we have to first Calculate the Initial Molarity of Molecules…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

A: Information about the question

Q: Suppose a 250. mL flask is filled with 0.20 mol of O₂ and 1.4 mol of NO. This reaction becomes…

A: The given equilibrium is N2 (g) + O2 (g) <----> 2 NO (g) Number of moles of O2 = 0.20 mol…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Given , Synthesis gas is mixture of carbon monoxide and water vapour. Volume of flask = 1.5 L

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

A: The detailed solution of the above question is given below;Explanation:

Q: Suppose a 250.mL flask is filled with 0.50mol of Cl2, 0.70mol of HCl and 2.0mol of CCl4. The…

A: A reaction is said to at equilibrium if the forward reaction rate is equal to the rate of backward…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: The final answer is :The pressure of Carbon di oxide is 0.39 atm.Explanation: Hope you got the…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Suppose a 500. mL flask is filled with 0.40 mol of N, and 0.90 mol of NH3. This reaction becomes…

A: volume of flask = 500 mL Initial moles of N2 and NH3 are 0.40 and 0.90 moles respectively.

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Carbon Tetrachloride can be produced by the following reaction: CS2 (g)+ 3 Cl2 (g)》S2 Cl2(g)+CCL4…

A: Given- Moles of CS2=1.20MMoles of Cl2=3.60 M Formulae used: Concentration = MolesVolume

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Answer: Value of equilibrium constant KP is equal to the ratio of partial pressure of product gases…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Br₂(g) + Cl₂(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 198.0 L flask initially contains 1.047 kg of…

A: The expression of equilibrium constant (in terms of partial pressure) in any reaction is Kp = Kc…

Q: Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.1 mol of NHz. This reaction becomes…

Q: Det a partial equilibrium. Sulfur dioxide and oxygen react to form sulfur trioxide during one of the…

Q: Suppose a 500. mL flask is filled with 0.10 mol of H₂ and 0.60 mol of HI. This reaction becomes…

A: Volume = 500 ml = 0.5 L Moles of H2= 0.10 mol Moles of HI = 0.60 mol

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Given: Volume=200mL At the beginning PCO=1.9 atmPH2O=3.8 atm After first equilibrium PCO=1.33…

Q: Consider the equilibrium system described by the chemical reaction below. A mixture of gas…

A: Information about the question

Q: alfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

A: Equilibrium constant is defined is ratio of partial pressure of products to the ratio of partial…

Q: Suppose a 250. mL flask is filled with 0.80 mol of O, and 0.30 mol of SO,. This reaction becomes…

A: Sulfur dioxide reacts with oxygen to form sulfur trioxide. The equation for the balanced chemical…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Answer:Given reaction:In the reaction, 2 moles of gases (1 mole CO and 1 mole H2O) are forming 2…

Q: Methanol and oxygen react to form carbon dioxide and water, like this: 2CH,OH(1)+30,(g)-2…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: "Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas…

A: Given data:Initial pressure of carbon monoxide = 0.88 atmInitial pressure of water vapor = 4.0…

Q: Suppose a 250. mL flask is filled with 1.2 mol of H₂ and 0.90 mol of HI. This reaction becomes…

Q: Suppose a 250. mL flask is filled with 1.4 mol of H₂ and 0.30 mol of HI. This reaction becomes…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

Q: Suppose a 250. mL flask is filled with 1.0 mol of N, and 2.0 mol of NH2. This reaction becomes…

Q: Suppose a 250. mL flask is filled with 0.30 mol of O, and 1.5 mol of NO. This reaction becomes…

A: Consider the given reaction as; N2 g + O2 g ⇌ 2 NO g Given information is as follows: Moles of O2 =…

Q: Steam reforming of methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and…

A: The chemical equation of steam reforming process is ; Expression for…

Q: While ethanol CH3CH2OH is produced naturally by fermentation, e.g. in beer- and wine-making,…

Q: Suppose a 250. mL flask is filled with 0.90 mol of H, and 0.40 mol of NH3. This reaction becomes…

Q: Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid…

A: The volume of the flask = 500 mLThe initial pressure of the sulfur dioxide gas = The initial…

Q: Consider the equilibrium system described by the chemical reaction below. A mixture of gas…

A: Given , Reaction : N2(g) +3H2(g) ⇌ 2NH3(g)

Question

100%

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 25.0 L tank with 6.9 mol of ethylene gas and 11. mol of water vapor. When the mixture has come to
equilibrium he determines that it contains 1.5 mol of ethylene gas and 5.6 mol of water vapor.
The engineer then adds another 2.8 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is
reached the second time. Round your answer to 2 significant digits.
I mol
Ox10

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Step 7

Step 8

Step 9

Trending now

This is a popular solution!

Step by step

Solved in 9 steps with 9 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 5.0 L flask with 1.0 atm of carbon monoxide gas and 2.5 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.69 atm of carbon monoxide gas, 2.19 atm of water vapor and 0.31 atm of hydrogen gas. The engineer then adds another 0.25 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
Suppose a 250. mL flask is filled with 0.40 mol of H₂ and 1.3 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H₂. You can leave out the M symbol for molarity. initial cha equilibrium H₂ 0 X 0 1₂ 0 HI 00 믐 X olo 18 Ar
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 500. mL flask with 0.82 atm of carbon monoxide gas and 0.85 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.33 atm of carbon monoxide gas, 0.36 atm of water vapor and 0.49 atm of hydrogen gas. The engineer then adds another 0.41 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 2.0 L flask with 3.1 atm of carbon monoxide gas and 3.6 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.0 atm of carbon monoxide gas, 1.5 atm of water vapor and 2.1 atm of carbon dioxide. The engineer then adds another 0.90 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. 0 atm x10 C [
While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene with water vapor at elevated temperatures. (CH,CH,) A chemical engineer studying this reaction fills a 75.0 L tank with 5.0 mol of ethylene gas and 20. mol of water vapor. When the equilibrium she determines that it contains 1.1 mol of ethylene gas and 16.1 mol of water vapor. mixture has come to The engineer then adds another 1.7 mol of ethylene, and allows the reached the second time. Round your answer to 2 significant digits. mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is I mol
Suppose a 500. mL flask is filled with 1.6 mol of H₂ and 0.30 mol of HI. This reaction becomes possible: H₂(g) + 12₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of I2. You can leave out the M symbol for molarity. initial change equilibrium H₂ 0 1₂ x 0 HI 0 X S
Suppose a 250. mL flask is filled with 0.60 mol of SO₂ and 1.0 mol of SO3. This reaction becomes possible: 2SO₂(g) + O₂(g) — 2SO3(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity. initial change equilibrium SO₂ 0₂ 0 X 0 SO₂ 0 010 X Ś
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 1.5L flask with 2.9 atm of carbon monoxide gas and 2.9 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.4 atm of carbon monoxide gas, 1.4 atm of water vapor and 1.5 atm of carbon dioxide. The engineer then adds another 0.97 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 Submit Assignment Continue 2021 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility MacBook Air DII 888 F10 F8 F9 esc F6 F7 F4 F5 F3 F2 %23 $4 % - & 4. 5 8.
Suppose a 500. mL flask is filled with 0.80 mol of I, and 1.0 mol of HI. This reaction becomes possible: H, (g) +1,(g) = 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of I,. You can leave out the M symbol for molarity. H, HI initial change equilibrium
"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 200. mL flask with 2.3 atm of carbon monoxide gas and 4.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.90 atm of carbon monoxide gas, 2.6 atm of water vapor and 1.4 atm of carbon dioxide. The engineer then adds another 1.0 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. 0 atm x10 X
A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) -> 2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b. If the container size is 3.0 L, what is the value of the equilibrium constant?
Suppose a 500. mL flask is filled with 1.4 mol of N, and 1.3 mol of NO. This reaction becomes possible: N,(2) +0,(2)- -2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N2 O2 NO initial change equilibrium olo