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## Main Question or Discussion Point

In reality pressure of a gas is lower than what is expected and volume is larger than expected - as ideal gas equation neglected volume of gas molecules and forces between them. Van der waal corrected it but:-

I need to know then why do we

Shouldnt we

similarly we should

Im a bit confused over van der waal's equation. Cannot understand it

I need to know then why do we

**add**the constant n^2a/V^2 in pressure and**subtract**nb in volumeShouldnt we

**subtract**n^2a/V^2 from pressure as it is lower than what was expectedsimilarly we should

**add**nb in volume as it is more than what was expectedIm a bit confused over van der waal's equation. Cannot understand it