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Compressibility factor, Z, of a gas is given as Z = pVnRT. What is the value of Z for an ideal gas? - Chemistry

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प्रश्न

Compressibility factor, Z, of a gas is given as Z = `(pV)/(nRT)`. What is the value of Z for an ideal gas?

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उत्तर

The value of Z for an ideal gas is 1. 

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पाठ 5: States of Matter - Multiple Choice Questions (Type - I) [पृष्ठ ५८]

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एनसीईआरटी एक्झांप्लर Chemistry [English] Class 11
पाठ 5 States of Matter
Multiple Choice Questions (Type - I) | Q 32.(i) | पृष्ठ ५८

संबंधित प्रश्‍न

Calculate the volume occupied by 8.8 g of CO2 at 31.1°C and 1 bar pressure. R = 0.083 bar L K–1 mol–1.


The value of the universal gas constant depends upon


Maximum deviation from ideal gas is expected from


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?


In what way real gases differ from ideal gases.


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.


Write the Van der Waals equation for a real gas. Explain the correction term for pressure and volume.


A plot of volume (V) versus temperature (T) for a gas at constant pressure is a straight line passing through the origin. The plots at different values of pressure are shown in Figure. Which of the following order of pressure is correct for this gas?


Compressibility factor, Z, of a gas is given as Z = `(pV)/(nRT)`. For real gas what will be the effect on value of Z above Boyle’s temperature?


Match the following graphs of ideal gas with their co-ordinates:

Graphical representation x and y co-ordinates
(i) (a) pV vs. V
(ii) (b) p vs. V
(iii) (c) p vs. `1/V`

Assertion (A): At constant temperature, pV vs V plot for real gases is not a straight line.

Reason (R): At high pressure all gases have \[\ce{Z}\] > 1 but at intermediate pressure most gases have \[\ce{Z}\] < 1.


Isotherms of carbon dioxide gas are shown in figure. Mark a path for changing gas into liquid such that only one phase (i.e., either a gas or a liquid) exists at any time during the change. Explain how the temperature, volume and pressure should be changed to carry out the change.


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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