At low pressure,the van der Waals equation be | vedclass

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Question

(C) The van der Waals equation for $1 \ mol$ of a gas is $(P + a/V_m^2)(V_m - b) = RT$. At low pressure,the volume $V_m$ is very large,so the term $b$

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$(P + a/V_m^2)(V_m) = RT$

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(C) The van der Waals equation for $1 \ mol$ of a gas is $(P + a/V_m^2)(V_m - b) = RT$. At low pressure,the volume $V_m$ is very large,so the term $b$ (which represents the excluded volume) becomes negligible compared to $V_m$,i.e.,$(V_m - b) \approx V_m$. Substituting this into the equation,we get $(P + a/V_m^2)(V_m) = RT$.

At low pressure,the van der Waals equation becomes

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