Consider the following equilibrium:2NH, ) - N, ) + 31H, )AG-34. JNow suppose a reaction vessel is filled with 0.691 atm of ammonia (NH,) and 9.56 atm of nitrogen (N,) at 1138. "C. Answer the following questionsabout this system:O riseUnder these conditions, will the pressure of NH, tend to rise or fall?O fallts it possible to reverse this tendency by adding H,?In other words, Iif you said the pressure of NH, wil tend to rise, can thatO yesbe changed to a tendency to fa by adding H, Simillarly, you said theO nopressure of NH, wil tend to fall, can that be changed to a tendency torise by adding H,If you said the tendency can be revensed in the second question, calculatethe minimum pressure of H, needed to reverse itRound your answer to 2 significant digits

Answered: Image /qna-images/answer/bd76e5cb-bbde-4425-bb09-50c27ae09063.jpg

Consider the following equilibrium: 2NH, Ge) -N, (e) + 31, e) AG-34. J Now suppose a reaction vessel is filled with 0.691 atm of ammonia (NH,) and 9.56 atm of nitrogen (N,) at 1138. "C. Answer the following questions about this system: se Under these cenditions, wil the pressure of NH, tend to re or fal? fall tst possible to reverse this tendency by adding H,? In other words, if you said the presture of NH, wi tend to rise, can that sa O One be changed to a tendency to fa by adding H, Smilarly, you said the pressure of NH, wi tend to fal, can that be changed to a tendency to rise by adding H, ar you said the tendency can be reversed in the second question, caloate the minimum pressure of H, needed to reverse it 0- Round your answer to 2 significant digits

Consider the following equilibrium: 2NH, Ge) -N, (e) + 31, e) AG-34. J Now suppose a reaction vessel is filled with 0.691 atm of ammonia (NH,) and 9.56 atm of nitrogen (N,) at 1138. "C. Answer the following questions about this system: se Under these cenditions, wil the pressure of NH, tend to re or fal? fall tst possible to reverse this tendency by adding H,? In other words, if you said the presture of NH, wi tend to rise, can that sa O One be changed to a tendency to fa by adding H, Smilarly, you said the pressure of NH, wi tend to fal, can that be changed to a tendency to rise by adding H, ar you said the tendency can be reversed in the second question, caloate the minimum pressure of H, needed to reverse it 0- Round your answer to 2 significant digits

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...

See similar textbooks

Similar questions

HYPOTHETICAL EQUILIBRIUM. NEED ASAP. DIRECTION: REMOVAL OF SOME N GIVE USED REFERENCES (IF THERE ARE)
3)Consider the reaction of decomposition of ammonia.The equilibrium of constant KC of this reaction at 400°C is 1.41 what is the equilibrium constant of reaction at the same temperature . this equation is in red
Consider the reaction: (see image) At the start of the reaction, the concentrations of the reactants and products are:[H2] = 0.100 M; [I2] = 0.100 M; [HI] = 0.000 M. At 427°C, the equilibriumconcentrations of the reactants and products are: [HI] = 0.158 M; [H2] = 0.021 M; [I2] = 0.021 M. Calculate the value of Keq for this reaction.
4. Sketch a graphical representation of the following events for the equilibrium below. PCI@ $ PCI® + Cl@ AH =+ 88 kJ/mol 5(g) a) PCl, is introduced into a flask at t=0 to a concentration of 2 mol/L. b) The flask is heated gently until no further changes in concentration of PCl, occur (5 minutes). At this time, the concentration of PCl(g) is 1.25 mol/L. c) At t=10 min an additional 0.25 mol/L of chlorine gas is injected into the flask. d) At t=15 min, no further changes in concentration were observed. e) Indicate the places on the graph where the system is at equilibrium. f) Use the information provided to calculate K, the equilibrium constant of this reactions.
Write the equilibrium expression, Kc, for the following chemical reaction. 2C6Ha(g) + 1502(g) * 12CO2(g) + 6H2O(g). [co.] [H,0] А. [co.]" [1,0] В. CH.] [0,] |co,] [1,0] C [co,]" [1,0] D.
Determine the direction of the equilibrium will shift to as a result of the following changes.
releasing heat lenerg 4. The following equilibrium is exothermic. How could the yield of diiodine pentoxide be increased? D. decreasing temp? I2(g) + 5CO₂(g) = 5CO(g) + 1205(g) A. by decreasing the pressure Bby increasing the pressure C. by decreasing the volume of the reaction vessel D. by decreasing the temperature E. by increasing the temperature
4. At 1000 K, 0.3 % of 1 mol ofL dissociates to establish the equilibrium represented by the equation, I2 (g) 2 21 (g), in one liter container. The value of Ke at 1000 K is: A) 3.6 x 105 B) 6.0 x 10-3 C) 3.7 x 10-3 D) 6.0 x 10 -5 E) 2.8 x 10 -3
The equilibrium constant, K., for the following reaction is 5.10x10 at 548 K. NH,CKs)ENH3(g) + HCKg) If an equilibrium mixture of the three compounds in a 7.05 L container at 548 K contains 1.62 mol of NHCKS) and 0.486 mol of NH, the aumber of moles of HCI present is moles.
(please type answer no write by hend)
K for the reaction of hydrogen and iodine to produce hydrogen iodide, H2(g) + I(g) = 2HI(g) is 54.3 at 430°C. Determine the initial and equilibrium concentration of HI if initial concentrations of H2 and I, are both 0.11 M and their equilibrium concentrations are both 0.054 M at 430°C. [HI); M %3D [HI). M %3D
[6] 0,40 mol pure sulfur trioxide is heated in a closed vessel and decomposes partially in sulfur dioxide and dioxygen. At 1000 K 0,10 mole dioxygen has been formed, all substances are gaseous and the volume of the gas mixture is 27 liter. a) Calculate the value of the equilibrium constant K. at 1000 K. b) Calculate the value of the equilibrium constant K, at 1000 K. c) Calculate the (degree of) dissociation of sulfur trioxide.