In the van der Waals model of a gas, as compared to an ideal gas, a....

In the van der Waals model of a gas, as compared to an ideal gas,

a. Intermolecular forces decrease the pressure, but finite molecular volume increases it

b. Both intermolecular forces and finite molecular volume increase the pressure

c. Both intermolecular forces and finite molecular volume decrease the pressure

d. Intermolecular forces increase the pressure, but finite molecular volume decreases it

Solutions

Expert Solution

For ideal gases, The particles have no attraction and repulsion for each other .

Whereas, real gases have interaction towards each other and they don't obey the ideal gas laws

Van der waal's equation for real gases is given by ,

(P + an²/V²)(V-nb) = nRT ,

Which shows that pressure of real gases is less than that of ideal gases.

So, the correct answer is :

C- Both intermolecular forces and finite molecular volume decreases the pressure.

queen_honey_blossom answered 1 year ago

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