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A piston-cylinder device contains a mixture of NO29) and N204g), which are in chemical equilibrium with the equilibrium constant Kp = 6.739 at a given T. a. At first the piston is adjusted to a Ptotal inside the cylinder of 2.00 atm. Determine the partial pressures and mole fractions of both gases inside the cylinder (assume ideal gas behavior). b. Assuming T=298 K, and a 5.0 liter container, 0.25 moles of NO2 and 0.25 moles of N204 are added. In which direction will the reaction become spontaneous? c. Two moles of Ar (inert gas) are added to the container, while keeping V & T constant. What are the final equilibrium pressures for each gas?

A piston-cylinder device contains a mixture of NO29) and N204g), which are in chemical equilibrium with the equilibrium constant Kp = 6.739 at a given T. a. At first the piston is adjusted to a Ptotal inside the cylinder of 2.00 atm. Determine the partial pressures and mole fractions of both gases inside the cylinder (assume ideal gas behavior). b. Assuming T=298 K, and a 5.0 liter container, 0.25 moles of NO2 and 0.25 moles of N204 are added. In which direction will the reaction become spontaneous? c. Two moles of Ar (inert gas) are added to the container, while keeping V & T constant. What are the final equilibrium pressures for each gas?

Chemistry
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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A piston-cylinder device contains a mixture of NO2(g) and N204(g), which are in chemical equilibrium with the equilibrium constant Kp = 6.739 at a given T. a. At first the piston is adjusted to a Ptotal inside the cylinder of 2.00 atm. Determine the partial pressures and mole fractions of both gases inside the cylinder (assume ideal gas behavior). b. Assuming T=298 K, and a 5.0 liter container, 0.25 moles of NO2 and 0.25 moles of N204 are added. In which direction will the reaction become spontaneous? c. Two moles of Ar (inert gas) are added to the container, while keeping V & T constant. What are the final equilibrium pressures for each gas?
Transcribed Image Text:A piston-cylinder device contains a mixture of NO2(g) and N204(g), which are in chemical equilibrium with the equilibrium constant Kp = 6.739 at a given T. a. At first the piston is adjusted to a Ptotal inside the cylinder of 2.00 atm. Determine the partial pressures and mole fractions of both gases inside the cylinder (assume ideal gas behavior). b. Assuming T=298 K, and a 5.0 liter container, 0.25 moles of NO2 and 0.25 moles of N204 are added. In which direction will the reaction become spontaneous? c. Two moles of Ar (inert gas) are added to the container, while keeping V & T constant. What are the final equilibrium pressures for each gas?
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