An analysis of the equilibrium mixture gives the following results:
SO3(g) 0.053mol, CO2(g) 0.106mol, CS2(g) 0.047mol, O2(g) 0.025mol.
Calculate K for this reaction (also give units of K).
5. At a particular temperature, 8.0mol NO2 is placed in a 1.0L container and the NO2 dissociates by the reaction:
2 NO2(g) <==> 2 NO(g) + 1 O2(g)
At equilibrium, 75% of NO has reacted. Calculate the equilibrium concentrations of all the species (called equilibrium position) and K (include units of K) for this reaction.
6. At a given temperature, the reaction below has a K = 2.50
1 SO2(g) + 1 NO2(g) <==> 1 SO3(g) + NO(g)
If all four gases had an initial concentration of 1.00M, calculate the equilibrium concentration of all species.
7. The industrial production of ammonia is described by this reversible reaction
1 N2(g) + 3 H2(g) <==> 2 NH3(g) + Energy
Using the 4 part explanation for how Le Chatlier's Principle would explain how the system would be affected by the following stresses:
a. addition of heat
b. removal of NH3
c. decrease of pressure
d. addition of a catalyst
Problem 4 : K = 9.89E-4 M2
Problem 5 : K = 0.11 M
Problem 6 : [SO3]E = 1.22M, [NO]E = 1.22M, [SO2]E = 0.776M, [NO2]E = 0.776M