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प्रश्न
561 dm3 of a gas at STP is filled in a 748 dm3 container. If the temperature is constant, calculate the percentage change in pressure required.
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उत्तर
Initial volume = V1 = 561 dm3
Final volume = V2 = 748 dm3
Difference in volume = 748 - 561 = 187 dm3
As the temperature is constant,
Decrease in pressure percentage = `187/748 xx 100 = 25%`
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संबंधित प्रश्न
Explain Boyle's Law on the basis of the kinetic theory of matter.
At constant temperature, the effect of change of pressure on the volume of a gas was as given below:
|
Pressure in atmosphere |
Volume in liters |
|
0.20 |
112 |
|
0.25 |
89.2 |
|
0.40 |
56.25 |
|
0.60 |
37.40 |
|
0.80 |
28.10 |
|
1.00 |
22.4 |
(a) Plot the following graphs
- P vs V
- P vs 1/V
- PV vs P
Interpret each graph in terms of the law.
(b) Assuming that the pressure values given above are correct, find the correct measurement of the volume.
A steel cylinder of internal volume 20 litres is filled with hydrogen at 29 atmospheric pressure. If hydrogen is used to fill a balloon at 1.25 atmospheric pressure at the same temperature, what volume will the gas occupy?
A gas at 240 K is heated to 127°C. Find the percentage change in the volume of the gas (pressure remaining constant).
At 0°C and 760 mmHg pressure, a gas occupies a volume of 100 cm3. Kelvin temperature of the gas is increased by one-fifth and the pressure is increased one and a half times. Calculate the final volume of the gas.
Calculate the volume occupied by 2 g of hydrogen at 27°C and 4-atmosphere pressure if at STP it occupies 22.4 litres.
State Boyle’s Law.
Correct the following statement:
The volume of a gas is inversely proportional to its pressure at a constant temperature.
Calculate the following:
Calculate the temperature at which a gas ‘A’ at 20°C having a volume, of 500 cc. will occupy a volume of 250 cc.
Assuming temperature remaining constant calculate the pressure of the gas in the following:
The pressure of a gas having volume 1000 cc. originally occupying 1500 cc. at 720 mm. pressure.
