aq) + 42CO2(g) + 24H2O(l)
1.
Increase the concentration of carbon dioxide.
2.
Argon gas is added.
3.
Increase the concentration of the Ce(IO3)4.
4.
Decrease the volume.
5.
Decrease the temperature (the reaction is exothermic).
6.
Decrease the concentration of the I2.
1. This would drive the equilibrium towards the production of more Ca(IO3)2(s) and less CO2(g) and H2O(l), according to Le Chatelier's principle.
2. Adding an inert gas like argon would not affect the equilibrium.
3. Increasing the concentration of Ce(IO3)4 would shift the equilibrium towards the production of more Ca(IO3)2(s) and I2(aq) to balance out the increased concentration of reactants.
4. Decreasing the volume would also increase the pressure, which would drive the equilibrium towards the production of less gaseous products, so more Ca(IO3)2(s) and less CO2(g) and H2O(l).
5. Decreasing the temperature would favor the exothermic direction of the reaction, producing more Ca(IO3)2(s), CO2(g) and H2O(l).
6. Decreasing the concentration of I2 would shift the equilibrium towards the production of more I2(aq) and Ca(IO3)2(s) to balance out the decreased concentration of reactant.