2. What is the final temperature of a gas when the volume at 15.0 degrees Celsius was
15 L and changed to 5.0 L if the pressure remains constant?

- 177°C

Explanation:

Data obtained from the question include:

V1 (initial volume) = 15L

T1 (initial temperature) = 15°C = 15 + 273 = 288K

V2 (final volume) = 5L

T2 (final temperature) =?

Since the pressure is constant, the gas is obeying Charles' law.

Using the Charles' law equation V1/T1 = V2/T2, the final temperature of the gas can be obtained as follow:

V1/T1 = V2/T2

15/288 = 5/T2

Cross multiply to express in linear form as shown below:

15 x T2 = 288 x 5

Divide both side by 15

T2 = (288 x 5)/15

T2 = 96K

Now, we need to convert 96K to celsius temperature. This is illustrated below

°C = K - 273

°C = 96 - 273

°C = - 177°C

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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.