Consider the following system at equilibrium. A(aq) = B(aq) AH = +350 kJ/mol What can be said about Q and K immediately after an increase in temperature? O Q < K because K increased. Q > K because Q increased. Q > K because K decreased. O Q< K because Q decreased. O Q = K because neither changed. How will the system respond to a temperature increase? shift left no change shift right

Use the following information to answer the next question Factors that can affect equilibrium I and II III only I, II, and III I. O II only II. III. The factors from the list above that would increase the equilibrium concentration of NO(g) in the system; 4NH3(g) +502 (g) 4NO(g) + 6H₂O(g) AH = -905 kJ while all other variables are held constant are Decreasing the volume Increasing the temperature Adding NH3(g)

For the following reaction 2 SO2(g) + O2(g)   <->   2 SO3(g)  +  heat If the equilibrium situation is stressed by increasing the volume of the container, the reaction will shift toward a No change b Right or products c Left or reactants

Consider the following equilibrium   If the equilibrium concentration of chlorine and phosphorous trichloride are 0.80 mol/L and 0.70 mol/L, respectively,find the equilibrium concentration of phosphorous pentachloride.

Phosphorus pentachloride decomposes at higher temperatures. PC15 (8) PCl3(g) + Cl₂(g) An equilibrium mixture at some temperature consists of 5.81 g PCI, 208.23 g/mol 4.86 g PC3, 137.33 g/mol 3.59 g Cl₂, 70.91 g/mol in a 1.00-L flask. If you add 1.31 g of Cl₂, how will the equilibrium be affected and what will the concentration of PCI, be when equilibrium is reestablished? O shift left O shift right Ono shift will occur [PCI5] = mol/L