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Compressibility factor for CO2 at 400 K and 71.0 bar is 0.8697. The molar volume of CO2 under these conditions is

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प्रश्न

Compressibility factor for CO2 at 400 K and 71.0 bar is 0.8697. The molar volume of CO2 under these conditions is

विकल्प

  • 22.04 dm3

  • 2.24 dm3

  • 0.41 dm3

  • 19.5 dm3

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उत्तर

0.41 dm3

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  क्या इस प्रश्न या उत्तर में कोई त्रुटि है?
अध्याय 6: Gaseous State - Evaluation [पृष्ठ १८०]

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सामाचीर कलवी Chemistry - Volume 1 and 2 [English] Class 11 TN Board
अध्याय 6 Gaseous State
Evaluation | Q I. 14. | पृष्ठ १८०

संबंधित प्रश्न

25 g of each of the following gases are taken at 27°C and 600 mm Hg pressure. Which of these will have the least volume?


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Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if it is compressed to a smaller volume at a constant temperature.


Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if more gas is introduced into the same volume and at the same temperature.


Which of the following gases would you expect to deviate from ideal behavior under conditions of low-temperature F2, Cl2, or Br2? Explain.


If 1 gram of each of the following gases are taken at STP, which of the gases will occupy (a) greatest volume and (b) smallest volume?

\[\ce{CO, H2O, CH4 , NO}\]


Pressure versus volume graph for a real gas and an ideal gas are shown in figure. Answer the following questions on the basis of this graph.

(i) Interpret the behaviour of real gas with respect to ideal gas at low pressure.

(ii) Interpret the behaviour of real gas with respect to ideal gas at high pressure.

(iii) Mark the pressure and volume by drawing a line at the point where real gas behaves as an ideal gas.


In van der Waal's equation for the real gas, the expression for the net force of attraction amongst the gas molecules is given by:


Choose the correct option for the total pressure (in atm.) in a mixture of 4g \[\ce{O2}\] and 2g \[\ce{H2}\] confined in a total volume of one litre at 0°C is ______.

[Given R = 0.082 L atm mol−1K−1, T = 273 K]


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