Why does Ce2(SO3)3 have a lower solubility than KCl?

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A saturated solution is at equilibrium (rate of dissolution is equal to rate of crystallization) with some equilibrium constant K1. If you change the temperature of the system at equilibrium, you will observe a different equilibrium constant K2. Whether the equilibrium constant increase or decreases is described by the Van't Hoff equation:

ln(K2K1)=−ΔHR(1T2−1T1)

So it depends on the sign of the enthalpy of reaction, in this case the enthalpy of dissolution.

according to kinetic-molecular theory, the following would not be considered an ideal gas:

a gas at very low volumes, when gas particles are very close together

a gas at very low temperatures, when gas particles have very little kinetic energy a gas

a gas with highly polar molecules that have very strong intermolecular forces

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