N2(g) + 3H2 (g) = 2NH3 (g) AH°pn =-92 kJ Which of the following changes would cause the value of K for this reaction to increase? You can choose any combination of answers. Decreasing the volume of the reaction container. Heating the reaction container Cooling the reaction container Adding Helg) to the reaction container removing NH3(g) from reaction container.

N2(g) + 3H2 (g) = 2NH3 (g) AH°pn =-92 kJ Which of the following changes would cause the value of K for this reaction to increase? You can choose any combination of answers. Decreasing the volume of the reaction container. Heating the reaction container Cooling the reaction container Adding Helg) to the reaction container removing NH3(g) from reaction container.

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

Consider the following equilibrium: N₂O4 (g) 2NO₂ (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 1.32 atm of dinitrogen tetroxide (N₂O4) at 322. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to 2 rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. O O 0 rise fall yes no atm x10 x Ś
Consider the following equilibrium: N₂(g) + 3H₂(g) → 2NH3 (g) Now suppose a reaction vessel is filled with 7.18 atm of nitrogen (N₂) and 0.0762 atm of ammonia (NH3) at 359. °C. Answer the following questions about this system: AGO= = -34. kJ Under these conditions, will the pressure of NH3 tend to rise or fall? H₂? Is it possible to reverse this tendency by adding 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. rise fall 0 yes O no atm x10 X
9. For the following reaction: 3 Fe (s) + 4 H2O (g) = Fe3O4 (s) + 4 H2 (g) Change in H = -150 kJ Will the position of equilibrium shift left towards reactants, shift right toward products, or not change if: A) More Fe3O4 (s) is added to the system B) The temperature is increased C) The volume of the container is increased D) A catalyst is added E) H2 (g) is added to the system
Which of the following is true about the following reaction when the temperature is raised? N₂O4(g) 2 NO₂(g) AH = 57.0 kJ Equilibrium will shift to the right. Equilibrium will shift to the left. Equilibrium will shift to produce more heat. No effect on the equilibrium.
Mercury(IT) oxide decomposes to form mercury and oxygen, like this: 2HgO(s)--2Hg(l)+O2(g) At a certain temperature, a chemist finds that a 3.5 L reaction vessel containing a mixture of mercury (It) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 15.3 g Hg 19.1 g O2 25.0 g Calculate the value of the equilibrium constant K, for this reaction, Round your answer to 2 significant digits.
Calculate the pressure of N2 needed to reverse the reaction (last row of the table. 0.38 is wrong). thank you!
Consider the following equilibrium: N₂ (g) + 3H₂ (g) 2NH3 (g) AG=-34. KJ Now suppose a reaction vessel filled with 3.73 atm of nitrogen (N₂) and 1.60 atm of ammonia (NH3) at 493. °C. Answer the following questions about this system: Under these conditions, will the pressure of N, tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of N₂ will tend to rise, can that be changed to a tendency to fall by adding H₂? Similarly, if you said the pressure of N₂ 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 significant digits. Ⓒrise fall O yes O no atm X S ? do Är
Consider the following equilibrium: N₂O4 (g) → 2NO₂ (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 0.399 atm of dinitrogen tetroxide (N₂O4) at 588. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. O O rise fall yes no atm x10 X 5
2 EMZ3(g) 2 EZ3(g) + M₂(g) AGxn-350 kJ/mol 17. A small sample of EMZ3 is placed into an evacuated, rigid metal container and allowed to reach equilibrium. Based on the value of AG and the chemical reaction, which of the following is true about the reaction? The value of K is much less than I and more products form than reactants
For the reaction N,(g) + 3 H, (g) = 2 NH,(g) a reaction mixture at a certain temperature contains N,, H,, and NH, in their standard states. If K, = 41, which statement is true of the reaction mixture? Qp > Kp; the reaction will proceed to the left. Qp < Kp; the reaction will proceed to the right. Q, = Kp; the reaction is at equilibrium.
7.B Consider the chemical equation C(s) + 2A(g) 5 2B(I) + heat. Be sure to briefly JUSTIFY each answer below. (a) Will SQUEEZING the container cause a disturbance to equilibrium? If so, then in what direction will the reaction occur? (b) Will RAISING THE TEMPERATURE of the system cause a disturbance to equilibrium? If so, then in what direction will the reaction occur? (c) What is the sign of the standard reaction ENTHALPY? Does the enthalpy change provide a favorable or unfavorable contribution to the spontaneity of the forward reaction at standard state conditions? (d) What is the sign of the standard reaction ENTROPY? Does the entropy change provide a favorable or unfavorable contribution to the spontaneity of the forward reaction at standard state conditions? (e) Based on (c,d) describe the preference for products or reactants at equilibrium at very LOW temperatures. (f) Based on (c,d) describe the preference for products or reactants at equilibrium at very HIGH temperatures.
Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (ΔrH= 40.5 kj/mol-rxn). N2O3 = NO +NO2 Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. increasing the volume of the reaction flask