At low pressure and high temperature, the Vander Waal’s equation is finally reduced (simplified) to :

Question

At low pressure and high temperature, the Vander Waal’s equation is finally reduced (simplified) to : (A) PVm = RT (B) (P + (a/Vm2)) (Vm - b ) = RT  (C) P(Vm - b) RT (D) (P + (a/Vm2))Vm = RT

Tardigrade Admin · Accepted Answer

At low pressure and high temperature, van der Waal's equation is modified as :

p V_{m} = RT

(for 1 mole )

∵

At low pressure and high temperature, the terms

\frac{a}{V ^{2}}

and

b

becomes very small as compared to

p

and

V

.

Q. At low pressure and high temperature, the Vander Waal’s equation is finally reduced (simplified) to :

$P V_{m} = RT$

$(P + \frac{a}{V _{m}^{2}}) (V_{m} - b) = RT$

$P (V_{m} - b) RT$

$(P + \frac{a}{V _{m}^{2}}) V_{m} = RT$

At low pressure and high temperature, van der Waal's equation is modified as :

$p V_{m} = RT$ (for 1 mole )

$∵$ At low pressure and high temperature, the terms

$\frac{a}{V ^{2}}$ and $b$ becomes very small as compared to $p$ and $V$ .

Q. At low pressure and high temperature, the Vander Waal’s equation is finally reduced (simplified) to :

PVm​=RT

(P+Vm2​a​)(Vm​−b)=RT

P(Vm​−b)RT

(P+Vm2​a​)Vm​=RT

At low pressure and high temperature, van der Waal's equation is modified as : pVm​=RT (for 1 mole ) ∵ At low pressure and high temperature, the terms V2a​ and b becomes very small as compared to p and V.

$P V_{m} = RT$

$(P + \frac{a}{V _{m}^{2}}) (V_{m} - b) = RT$

$P (V_{m} - b) RT$

$(P + \frac{a}{V _{m}^{2}}) V_{m} = RT$

At low pressure and high temperature, van der Waal's equation is modified as :

$p V_{m} = RT$ (for 1 mole )

$∵$ At low pressure and high temperature, the terms

$\frac{a}{V ^{2}}$ and $b$ becomes very small as compared to $p$ and $V$ .