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प्रश्न
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?
\[\ce{CO, H2O, CH4 , NO}\]
उत्तर
Molar volume of a gas is volume occupied by 1 mole of gas at STP (273.15 K and 1 bar pressure) and is equal to 22700 mL.
28 g of \[\ce{CO}\] occupy volume = 227000 mL
∴ 1 g of CO occupies volume = `22700/28` mL at STP
Similarly, 1 g of \[\ce{H2O}\] occupies volume = `22700/18` mL at STP
1 g of \[\ce{CH4}\] occupies volume = `22700/16` mL at STP
1 g of \[\ce{NO}\] occupies volume = `22700/30` mL at STP
(a) \[\ce{CH4}\] occupies greatest volume.
(b) \[\ce{NO}\] occupies smallest volume.
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संबंधित प्रश्न
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Compressibility factor, Z, of a gas is given as Z = `(pV)/(nRT)`. What is the value of Z for an ideal 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.
