If a 1.00-l container was rated to withstand pressures up to 25.0 atm, calculate what the temperature must have been when it ruptured. the final volume of the gas at 1.00 atm and 30°c was 55.0 l

a. 394°c

b. 667°c

c. no right choice.

C. No right choice

Explanation:

Using the gas equation:

V₁ P₁/T₁ =V₂ P₂/T₂ (1)

V₁= 1.00L

P₁= 25.0 atm

T₁= ?

V₂ = 55.0L

P₂ = 1.00 atm

T₂= 30°C

  =  303°K

Making T₁ in equation (1) subject of the formula;

T₁=(V₁ P₁/V₂ P₂)x  T₂ (2)

Substituting  into equation (2), we have:

T₁ =  [(1 x 25) / (55 x 1)] x 303

   = 137.7° K

  =   -135.27 ° C

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.