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प्रश्न
Assuming temperature remaining constant calculate the pressure of the gas in the following:
The pressure of a gas having volume 1800 ml. originally occupying 300 ml. at 6 atms. pressure.
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उत्तर
V1 = 300 ml
P1 = 6 atm.
V2 = 1800 ml
P2 = ?
At constant temperature P1V1 = P2V2
∴ P2 = `("P"_1"V"_1)/"V"_2 = (6 xx 300)/(1800) = 1`atm.
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संबंधित प्रश्न
State the law which is represented by the following graph:
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 certain mass of a gas occupies 2 litres at 27°C and 100 Pa. Find the temperature when volume and pressure become half of their initial values.
Calculate the volume occupied by 2 g of hydrogen at 27°C and 4-atmosphere pressure if at STP it occupies 22.4 litres.
Give its
(i) mathematical expression
(ii) graphical representation and
(iii) significance.
50 cm3 of hydrogen is collected over water at 17°C and 750 mmHg pressure. Calculate the volume of a dry gas at STP. The water vapour pressure at 17°C is 14 mmHg.
Calculate the following:
A gas ‘X’ is collected over water at 17°C and 750 mm. pressure. If the volume of the gas collected is 50 cc., calculate the volume of the dry gas at s.t.p. [at 17°C the vapour pressure is 14 mm.]
Fill in the blank with the correct word, from the words in option:
1 dm3 of a gas is equal to _______.
State-the law of volume
The following question refers to one mole of chlorine gas.
What will happen to volume of gas, if pressure is doubled?
