Advertisements
Advertisements
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?
\[\ce{CO, H2O, CH4 , NO}\]
Advertisements
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.
APPEARS IN
संबंधित प्रश्न
Which of the following is the correct expression for the equation of state of van der Waals gas?
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.
Can a Van der Waals gas with a = 0 be liquefied? explain.
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 the temperature is raised while keeping the volume constant.
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.
Write the Van der Waals equation for a real gas. Explain the correction term for pressure and volume.
Value of universal gas constant (R) is same for all gases. What is its physical significance?
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]
