A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -7 N2(g) + 3 H,(g)=2 NH3(g) к, — 6. х 10 He fills a reaction vessel at this temperature with 12. atm of nitrogen gas and 11. atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes x10 tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NH, at right. || atm Round your answer to 1 significant digit.

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -7 N2(g) + 3 H,(g)=2 NH3(g) к, — 6. х 10 He fills a reaction vessel at this temperature with 12. atm of nitrogen gas and 11. atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes x10 tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NH, at right. || atm Round your answer to 1 significant digit.

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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I am confused because I am getting two possible answers one being 10. 6 and the other being 1.38
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Suppose a 250.mL flask is filled with 1.6mol of Cl2, 1.3mol of HCl and 2.0mol of CCl4. The following reaction becomes possible: Cl2(g)+CHCl3(g)=HCl(g)+CCl4(g) The equilibrium constant K for this reaction is 8.61 at the temperature of the flask. Calculate the equilibrium molarity of CHCl3 . Round your answer to two decimal places.
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Suppose a 500. mL flask is filled with 0.50 mol of Cl₂, 1.7 mol of HCl and 0.20 mol of CC14. The following reaction becomes possible: Cl,(g)+CHCI, (g) → HCI(g) +CCI, (g) 4 The equilibrium constant K for this reaction is 0.104 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places.
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A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N, (g) + 3 H, (g) = 2 NH3 (g) К, — 3. х 10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 3.2 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes x10 tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.