Consider the following system at equilibrium where AH° = 198 kJ, and K = 0.0290, at 1150 K: 2SO3 (9)2S02 (9) + O2(9) If the VOLUME on the equilibrium system is suddenly decreased at constant temperature: The value of K O increases O decreases O remains the same The value of Qc O is greater than K O is equal to K O is less than K. The reaction must O run in the forward direction to reestablish equilibrium. Orun in the reverse direction to reestablish equilibrium. O remain the same. It is already at equilibrium. The number of moles of O2 will O increase O decrease remain the same

At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?

For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?

The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.

The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?

At 500C, k for the for the formation of ammonia from nitrogen and hydrogen gases is 1.5105. N2(g)+3H2(g)2NH3(g)Calculate the equilibrium partial pressure of hydrogen if the equilibrium partial pressures of ammonia and nitrogen are 0.015 atm and 1.2 atm, respectively.

For the given chemical equilibrium, these data are determined experimentally: T K 350K 3.76102 450K 1.86101 Determine H for this reaction.

For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of C at 1273 K, will the equilibrium mixture contain (a) mostly CO2? (b) mostly CO? (c) roughly equal amounts of CO2 and CO? (d) only C?

Consider the following system at equilibrium at 25C: PCl3(g)+Cl(g)PCl5(g)G=92.50KJ What will happen to the ratio of partial pressure of PCl5 to partial pressure of PCI3 if the temperature is raised? Explain completely.

The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.