What partial pressure of c2h4 gas (in mm hg) is required to maintain a solubility of 4.92×10-2 g/l in water at 25 °c? kh for c2h4 at 25 °c is 4.78×10-3 mol/l·atm.

The partial pressure of is 281 mmHg

Explanation:

We are given:

Solubility of ethene gas =

To convert this solubility into mol/L, we divide the given solubility by the molar mass of the gas, which is 28 g/mol

To calculate the molar solubility, we use the equation given by Henry's law, which is:

where,

= Henry's constant =

= molar solubility of ethene gas =

Putting values in above equation, we get:

Converting this into mmHg, we use the conversion factor:

1 atm = 760 mmHg

So,

Hence, the partial pressure of is 281 mmHg

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.