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Standard XII

Chemistry

Pressure and Temperature

In van der Wa...

Question

In van der Waals equation at constant temperature $300 K$ , if $a = 1.4 a t m L^{2} m o l^{- 2}$ , $V = 100 m L$ , $n = 1 m o l$ , then what is the pressure of the gas?

42 a t m

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210 a t m

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500 a t m

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106 a t m

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Solution

The correct option is D $106 a t m$
At moderate pressure van der Waals equation is given as :
$(P + \frac{a n^{2}}{V^{2}}) (V) = n R T$
$(P + \frac{1.4}{(0.1)^{2}}) (0.1) = 1 \times 0.082 \times 300$
Solving,
$P = 106 a t m$

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In van der Waals equation at constant temperature 300 K, if a=1.4 atm L2 mol−2, V=100 mL, n=1 mol, then what is the pressure of the gas?

The correct option is D 106 atmAt moderate pressure van der Waals equation is given as : (P+an2V2)(V)=nRT (P+1.4(0.1)2)(0.1)=1×0.082×300 Solving, P=106 atm

In van der Waals equation at constant temperature $300 K$ , if $a = 1.4 a t m L^{2} m o l^{- 2}$ , $V = 100 m L$ , $n = 1 m o l$ , then what is the pressure of the gas?

The correct option is D $106 a t m$
At moderate pressure van der Waals equation is given as :
$(P + \frac{a n^{2}}{V^{2}}) (V) = n R T$
$(P + \frac{1.4}{(0.1)^{2}}) (0.1) = 1 \times 0.082 \times 300$
Solving,
$P = 106 a t m$