At a certain temperature, 0.378 mol CH and 0.706 mol H2S are placed in a 1.50 L container.CH2(g) + 2H2S(g) CS2(g) + 4H2(g)At equilibrium, 12.3 g CS2 is present. Calculate Kc.Ke=

Step 1: The equilibrium constant (KC) is the ratio of the concentrations of gaseous (or aqueous)…

Answered: At a certain temperature, 0.378 mol CH…

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

Consider the following equilibrium: N₂O4(g) = 2NO2(g) A 1.00 L container is initially filled with 0.200 mol N₂O4At equilibrium, 0.160 mol NO₂are present. What is the equilibrium concentration of N₂O4? 0.120 mol/L 0. 040 mol/L O.0.160 mol/L 0.080 mol/L 0.100 mol/L
C6-6
8.2 mol NH3 are placed in a 10.5 L container at some temperature and allowed to come to equilibrium as per the reaction below. At equilibrium, 2.2 moles remained. What is the value of Kc for the following reaction at the temperature of the experiment? 2 NH3(g) N2(g) + 3 H2(g)
"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 25 L tank with 11. mol of carbon monoxide gas and 12. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.9 mol of carbon monoxide gas, 7.9 mol of water vapor and 4.1 mol of hydrogen gas. The engineer then adds another 3.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol
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
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 100 L tank with 45. mol of ethylene gas and 35. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 34. mol of ethylene gas and 24. mol of water vapor. The engineer then adds another 18. 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. | mol
Macmillan Learning At a certain temperature, 0.800 mol SO3 is placed in a 2.00 L container. 2 SO3(g) 2 SO₂(g) + O₂(g) At equilibrium, 0.200 mol O₂ is present. Calculate Ke. Kc = 0.040
While ethanol (CH₂CH₂OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH₂CH₂) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 75 L tank with 17. mol of ethylene gas and 13. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 7.9 mol of ethylene gas and 3.9 mol of water vapor. The engineer then adds another 3.3 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. mol x10 Ś
3sa
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 =
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
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)↽−−⇀CS2(g) ?c=9.40 at 900 K How many grams of CS2(g) can be prepared by heating 12.5 mol S2(g) with excess carbon in a 6.05 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g): g

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

At a certain temperature, 0.378 mol CH and 0.706 mol H2S are placed in a 1.50 L container. CH2(g) + 2H2S(g) CS2(g) + 4H2(g) At equilibrium, 12.3 g CS2 is present. Calculate Kc. Ke=