Consider the following equilibrium
2SO2(g) + O2(g) ⇔ 2SO3(g) DH=-197.78 kJ
- Write the
expression for the equilibrium constant, Kc, for this
- A mixture of SO2(g),
O2(g) and SO3(g) at 852K is allowed to reach
equilibrium. The concentrations at equilibrium are found to be:
[SO2] = 3.61 × 10-3 mol/L, [O2] = 6.11 × 10-4 mol/L, [SO3] = 1.01 × 10-3 mol/L.
Calculate the equilibrium constant, Kc for the system at 852K, including the correct units.
- What would be
the effect on the concentration of O2(g) and the value of Kc,
if the following changes were made to the system described above. For your
answer use “I” for increase, “D” for decrease and “R” for remains the same.
| || || [O2]
||Some SO3(g) is removed from the system ||________ ||_________|
||The volume is lowered at constant temperature, raising the pressure. ||________ ||_________|
||The temperature of the system is raised ||________ ||_________|
||A catalyst is added ||________ ||_________|
||Helium is added to the system ||________ ||_________|
||Some SO2(g) is added to the system ||________ ||_________|
||A small piece of Mg is ignited in the flask, after which the temperature is returned to 852K ||________ ||_________|
- At a different
temperature, the equilibrium constant, Kc, for this system
would be 963. In an equilibrium mixture at the new temperature [O2]
= 0.463 mol/L, and [SO3] = 0.821 mol/L. Calculate the concentration
of SO2 in the system.
- At the
temperature mentioned in d), a previously empty 5.00L flask is prepared by
adding 1.20 mol of SO2 and 1.50 mol of O2. Determine the
concentrations of SO2, O2 and SO3 once
equilibrium is established.
yet a third temperature, the Kc for this system would be 4.20 × 10-2. Initially a mixture at equilibrium in a 1.00 L flask
contains the following concentrations
[SO2] = 1.40 mol/L, [O2]
= 11.00mol/L, and [SO3] = 0.906 mol/L.
If an additional 2.00 moles of O2
are added to the flask, what will be the concentrations of the SO2,
O2 and SO3 once equilibrium is reestablished?
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Last Revised: March 17, 2004