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

Consider the following equilibrium: N2 g) +3H, (g) =2NH3 (g) AG" = - 34. kJ Now suppose a reaction vessel is filled with 4.68 atm of nitrogen (N, and 2.51 atm of ammonia (NH,) at 260. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? 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 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 rise by adding H2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. || atm Round your answer to 2 significant digits. O O

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.

For the reaction 2NO(g) + O2(g)- →2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 350.0 K is Assume that AH° and AS° are independent of temperature.

Consider the following system at equilibrium where AH° = -18.8 kJ/mol, and Kc = 10.5, at 350 K. 2 CH₂Cl₂ (9) CH4 (9) + CCI4 (9) When 0.33 moles of CH₂Cl₂ (g) are removed from the equilibrium system at constant temperature: The value of Kc The value of Qc Kc. 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 equilibrium. The concentration of CH4 will

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.

For the reaction N2(g) + 3H2(g)–→2NH3(g) AH° = -92.2 kJ and AS° = -198.7 J/K %3D The equilibrium constant for this reaction at 294.0 K is Assume that AH° and AS° are independent of temperature.

physical chem