Consider the following equilibrium: N, (e)+3H, (e)2NH, (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: rise fall 5 Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. yes no atm

Consider the following equilibrium: N, (e)+3H, (e)2NH, (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: rise fall 5 Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H₂ needed to reverse it. Round your answer to 2 significant digits. yes no 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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Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp: 109 at 298 K. If the equilibrium partial pressures of Br2 and NOBR at 0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at equilibrium... %D 2 NO(g) + Br2(g) = 2 NOBr(g) 1 NEXT へ If (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to solve for the partial pressure. Do not combine or simplify terms.. Kp 109 %3D RESET (109) (0.0159) (0.0768) 2(0.0159) 2(0.0768) (0.0159)? (0.0768)² (x) (2x) (x)? (2x)?
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Consider the following equilibrium: 2NH3 (g) = N2 (g)+ 3H, (g) AG = 34. kJ Now suppose a reaction vessel is filled with 7.65 atm of ammonia (NH,) and 0.884 atm of hydrogen (H,) at 600. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,? In other words, if you said the pressure of NH, will tend to rise, can that O yes be changed to a tendency to fall by adding N,? Similarly, if you said the O no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding N,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N, needed to reverse it. ||atm Round your answer to 2 significant digits.
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