Of the following equilibria, only will shift to the right in response to a decrease in volume. N2 (g) + 3H2 (g) 2NH3 (g) 2 Fe2O3 (s) 4 Fe (s) + 3O2 (g) 2 SO3 (g) 2 SO2 (g) + O2 (g) H2 (g) + Cl2 (g) 2 HCl (g) 2HI (g) H2 (g) + I2 (g)

Of the following equilibria, only one will shift to the right in response to a decrease in volume.

On decreasing the volume the equilibrium will shift in right direction due to less number of gaseous moles on product side.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

Decrease the volume

If the volume of the container is decreased , the pressure will increase according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. So, the equilibrium will shift in the direction number of gaseous moles are less.

On decreasing the volume the equilibrium will shift in right direction due to less number of gaseous moles on product side.

On decreasing the volume the equilibrium will shift in left direction due to less number of gaseous moles on reactant side.

On decreasing the volume the equilibrium will shift in left direction due to less number of gaseous moles on reactant side.

On decreasing the volume the equilibrium will shift in no direction due to same number of gaseous moles on both sides.

On decreasing the volume the equilibrium will shift in no direction due to same number of gaseous moles on both sides.

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.