For the reaction NH3 (g) + H2S (G) <----> NH4HS (s) K = 400. at 35.0°C. If 2.50 moles each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium? Mass = _______ g Pressure = _______ atm
For the reaction NH3 (g) + H2S (G) <----> NH4HS (s) K = 400. at 35.0°C. If 2.50 moles each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium? Mass = _______ g Pressure = _______ atm
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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For the reaction
NH3 (g) + H2S (G) <----> NH4HS (s)
K = 400. at 35.0°C. If 2.50 moles each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium?
Mass = _______ g
Pressure = _______ atm
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