Match each of the given equilibrium constants with the reaction spontaneity: K= 51.18 K=1 K = 0.00727 K= -5.23 This is not a valid equilibrium constant At equilibrium Spontaneous reverse Spontaneous forward

FaceboOK [Review Topics] [References) Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° 268 kJ, and K. 5.10x106, at 548 K. %3D NH,CI(s) NH3(g) + HCI(g) When some moles of NH,CI(s) are removed from the equilibrium system at constant temperature: The value of K The value of Q. The reaction must O run in the forward direction to restablish equilibrium. O run in the reverse direction to restablish equilibrium. O remain the same. It is already at cquilibrium. The concentration of NH, will Retry Entire Group 1 more group attempt remaining Submit Answer

For the equilibrium: 2F, (g) + O2 (g) + 600 kJ = 20F2 (g) where ke= 350 %3D What would be impact of decreasing the size of the reaction chamber? the quantity of F2(g) would increase energy would be absorbed by the reaction as the equilibrium shifts right adding Helium gas the quantity of OF,(g) would increase

Consider the decomposition reaction at 555 K   4POCl3 (g)    P4  (g) + 2O2  (g) + 6Cl2  (g)   If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm.  Find Kp and Kc.

Consider the following equilibrium: 2NH, (g) - N, (g)+3H, (g) AG° = 34. kJ Now suppose a reaction vessel is filled with 4.89 atm of ammonia (NH,) and 5.72 atm of nitrogen (N,) at 847. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding H,? In other words, if you said the pressure of NH, will tend to rise, can that 3 yes be changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of NH, will tend to fall, can that be changed to a tendency to 3 rise by adding H,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. 2. atm Round your answer to 2 significant digits.

physical chem

Consider the following equilibrium: 2NOC1 (g) 2NO(g) + Cl₂ (g) AG=41. KJ Now suppose a reaction vessel is filled with 3.76 atm of nitrosyl chloride (NOC1) and 6.26 atm of nitrogen monoxide (NO) at 1161. °C. Answer the following questions about this system: Under these conditions, will the pressure of NO tend to rise or fall? Is it possible to reverse this tendency by adding C1₂? In other words, if you said the pressure of NO will tend to rise, can that be changed to a tendency to fall by adding C1₂? Similarly, if you said the pressure of NO will tend to fall, can that be changed to a tendency to rise by adding Cl₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of C12 needed to reverse it. Round your answer to 2 significant digits. OO rise fall yes no atm x10 X Ś

A] HgS occurs in two crystalline forms called "red" and "black". For the conversion of 8. L- the red form to the black form at 525 °C, 4Gº = -0.157 kJ mol-¹ and AH = 4.184 kJ mol-¹. Assuming the AH is temperature independent, find the temperature at which the two forms can coexist at equilibrium at 1.000 bar. Which is more stable above this temperature?

Consider the following system at equilibrium where Ho = 18.8 kJ, and Kc = 9.52E-2, at 350 K: CH4(g) + CCl4(g) 2 CH2Cl2(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature:   whats the value of Kc   The value of Q   The reaction must

[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH=-108 kJ, and K. 77.5, at 600 K. CO(g) + C,(g) COCI,(g) When 0.22 moles of Cl,(g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish cquilibrium. O remain the same. It is already at cquilibrium. The concentration of CO will Submit Answer Retry Entire Group 1 more group attempt remaining