Consider the following system at equilibrium where AH = 92.7 kJ and Ke = 1.80 x 10-4, at 298 K. NH4HS(s) NH3(g) + H₂S(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: increasing the pressure (by changing the volume): decreasing the volume: adding NH4HS: adding H₂S: V

Consider the following system at equilibrium where AH = 92.7 kJ and Ke = 1.80 x 10-4, at 298 K. NH4HS(s) NH3(g) + H₂S(9) The production of NH3(g) is favored by (indicate true or false): decreasing the temperature: increasing the pressure (by changing the volume): decreasing the volume: adding NH4HS: adding H₂S: V

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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Consider the following equilibrium: 2NO₂(g) → N₂O4 (g) AG = -5.4 kJ Now suppose a reaction vessel is filled with 0.202 atm of nitrogen dioxide (NO₂) at 504. °C. A Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O4? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O4? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O4? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O needed to reverse it. V Round your answer to 2 significant digits. Orise fall O yes no atm 0
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