Consider the above reaction. If some CO2 were removed from the container, what would the reaction do in an attempt to replace the CO2?

See explanation

Explanation:

The reaction to be considered is shown below;

H2CO3<>CO2 + H2O

We know  that when a constraint such as a sudden change in concentration, pressure or temperature is imposed on  a reaction system in equilibrium, the system has to adjust itself by shifting in a particular direction in order to cancel the constraint.

Now, if we remove CO2, the equilibrium position must shift to the right by the decomposition of more H2CO3 to establish equilibrium again.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.