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Standard XII

Physics

Specific Heat Capacity

The compressi...

Question

The compressibilty factor of $N_{2}$ at 330K & 800 atm is 1.90 and at 570K & 200 atm is 1.10. A certain mass of $N_{2}$ occupies a volume of $1 d m^{3}$ at 330K and 800 atm. Calculate the volume of $N_{2}$ gas at 570K and 200 atm:

1 L

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2 L

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3 L

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4 L

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Solution

The correct option is D 4 L
$Z = \frac{P V_{m}}{n R T} \Rightarrow 1.9 = \frac{1 \times 800}{n \times R \times 330}$
$n = \frac{1 \times 800}{1.9 R \times 330}$
$Z = 1.1 = \frac{V \times 200}{n R \times 570}$
$V = 4 L$

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Similar questions

Q. The compressibility factor of

N_{2}

at & 800 atm is 1.90 and at 570K & 200 atm is 1.10. A certain mass if

N_{2}

occupies a volume of

{1 d m}^{3}

at 330K and 800 atm. Calculate the volume of

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gas at 570K and 200 atm.

Q. The compressibility factor of

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at 330K and 800 atm is 1.90 and at 570K and 200 atm is 1.10. A certain mass of

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1 {d m}^{3}

at 330K and 800 atm. Calculate the volume of

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Q. The compressibility factor of nitrogen at 330 K and 800 atm is 1.90 and at 570 K and 200 atm is 1.10. A certain mass of

N_{2}

occupies a volume of 1

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at 330 K and 800 atm. Calculate the volume occupied by the same quantity of

N_{2}

gas at

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Q. The compressibilty factor of

N_{2}

at 330 K & 800 atm is 1.90 and at 570 K & 200 atm is 1.10 A certain mass of

N_{2}

occupies a volume of 1

d m^{3}

at 330 K and 800 atm. Calculate the volume of

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gas at 570 K and 200 atm :

The compressibility factor for nitrogen at 330 K and 800 atm is 1.90 and at 570 K and 200 atm is 1.10. A certain mass of $N_{2}$ occupies a volume of 1 $d m^{3}$ at 330 K and 800 atm. Calculate the volume occupied by same quantity of $N_{2}$ gas at 750 K and 200 atm.

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The compressibilty factor of N2 at 330K & 800 atm is 1.90 and at 570K & 200 atm is 1.10. A certain mass of N2 occupies a volume of 1dm3 at 330K and 800 atm. Calculate the volume of N2 gas at 570K and 200 atm:

The correct option is D 4 LZ=PVmnRT⇒1.9=1×800n×R×330n=1×8001.9R×330Z=1.1=V×200nR×570V=4L

The compressibilty factor of $N_{2}$ at 330K & 800 atm is 1.90 and at 570K & 200 atm is 1.10. A certain mass of $N_{2}$ occupies a volume of $1 d m^{3}$ at 330K and 800 atm. Calculate the volume of $N_{2}$ gas at 570K and 200 atm:

The correct option is D 4 L
$Z = \frac{P V_{m}}{n R T} \Rightarrow 1.9 = \frac{1 \times 800}{n \times R \times 330}$
$n = \frac{1 \times 800}{1.9 R \times 330}$
$Z = 1.1 = \frac{V \times 200}{n R \times 570}$
$V = 4 L$