Methane (CH4, molar mass = 16.0 g/mol) has a Henry's Law constant (kH) of 9.88 × 10–2 mol/(L·atm) when dissolved in benzene at 25 °C. How many grams of CH4will dissolve in 3.00 L of benzene if the partial pressure of CH4 is 1.48 atm?

The mass of methane that will dissolve is 0.7008 grams

Explanation:

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

where,

= Henry's constant =

= molar solubility of methane gas = ?

= partial pressure of methane gas = 1.48 atm

Putting values in above equation, we get:

To calculate the mass of solute, we use the equation used to calculate the molarity of solution:

Given mass of methane = ?

Molar mass of methane = 16.0 g/mol

Molarity of solution = 0.0146 M

Volume of solution = 3.00 L

Putting values in above equation, we get:

Hence, the mass of methane that will dissolve is 0.7008 grams

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.

i don't see a text, but i am gonna assume this *orbit* the curved path, usually elliptical, described by a planet, satellite, spaceship, etc., around a celestial body, as the sun.