Compound A has a stronger intermolecular force between its molecules than compou

Question

Compound A has a stronger intermolecular force between its molecules than compound B. Both compounds are in the liquid state. Which compound will have a higher normal boiling point? Which compound will have a lower vapor pressure? Which compound will have a lower heat of vaporization? b) Which one of the following would have the lowest boiling point? A) Ar B) He C) Kr D) Ne E) Xe c) Which one of the following would have the lowest freezing point? A) pure H_2O B) 1 M KCl C) 1 M NaNO_3 D) 1 M Na_2SO_4 d) Br_2 molecules are held together in the liquid state due to: A) Dipole-dipole forces C) Hydrogen bonding B) London dispersion forces D) Ion-dipole forces e) Which one of the following solutions would have the lowest vapor pressure? A) 1 m C_6H_12O_6 B) 1 m MgCl_2 C) 1 m NaNO_3 D) 1 m NaBr

Explanation / Answer

17 a) i) Compound A has higher normal boiling point as it has stronger intermolecular forces which tightly held the molecules together.
ii) Compound A has lower vapor pressure as it has higher boiling point.
iii) Compound B has lower heat of vaporisation as it has comparitively weaker intermolecular forces.

b) B) He has lowest boiling point as it has weakest van der waals forces of attraction due to lowest polarisability and highest ionisation energy.

c) D) 1 M Na2SO4 has lowest freezing point as it gives maximum number of ions in solution. 1 molecule of na2SO4 ionises to give 3 ions.

d) Br2 molecules are held toghether in the liquid state due to very weak B) London dispersion forces (van der waals forces of attraction) as Br2 is a non polar molecule.

e) 1 m MgCl2 would have the lowest vapour pressure as it gives maximum number of ions in solution. 1 molecule of MgCl2 dissociates to give 3 ions.

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