Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.1 mol of NH2. This reaction becomes possible: N, (g) + 3H,(g) – 2NH, (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. 圖 Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N, H, NH, initial change equilibrium 미 ×

Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.1 mol of NH2. This reaction becomes possible: N, (g) + 3H,(g) – 2NH, (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. 圖 Use x to stand for the unknown change in the molarity of N,. You can leave out the M symbol for molarity. N, H, NH, initial change equilibrium 미 ×

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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Suppose a 250. mL flask is filled with 1.6 mol of NO and 0.40 mol of NO,. The following reaction becomes possible: NO3 (g) + NO (g) → 2 NO, (g) The equilibrium constant K for this reaction is 0.225 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places.
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Suppose a 250. mL flask is filled with 1.2 mol of OCl,, 1.9 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br,(g) +OCl,(g) BROCI(g) +BrC1(g) The equilibrium constant K for this reaction is 1.94 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.2 mol of Br,, 1.4 mol of OCl, and 1.1 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g) - BrOC1 (g) +BrC1(g) The equilibrium constant K for this reaction is 0.483 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. OM
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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
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