Advertisements
Advertisements
प्रश्न
2 liters of gas is enclosed in a vessel at a pressure of 760 mmHg. If the temperature remains constant, calculate pressure when volume changes to 4 dm3.
Advertisements
उत्तर
V = 2 litres
P = 760 mm
V1 = 4000 m3 [1 dm3 = 4 litres]
P1= ?
`"PV"/"T" = ("P"_1 "V"_1)/"T"_1`
`(760 xx 2)/"T" = ("P"_1 xx 4)/"T"_1`
`"P"_1 = 760/2 = 380` mm
APPEARS IN
संबंधित प्रश्न
Give the assumptions of the kinetic molecular theory.
State the law which is represented by the following graph:
Calculate the final volume of a gas 'X' if the original pressure of the gas at STP is doubled and its temperature is increased three times.
An LPG cylinder can withstand a pressure of 14.9 atmospheres. The pressure gauge of the cylinder indicates 12 atmospheres at 27°C. Because of a sudden fire in the building, the temperature rises. At what temperature will the cylinder explode?
State Charles's law.
A certain mass of gas occupied 850 ml at a pressure of 760 mm of Hg. On increasing the pressure it was found that the volume of the gas was 75% of its initial value. Assuming constant temperature, find the final pressure of the gas?
It is required to reduce the volume of a gas by 20% by compressing it at a constant pressure. To do so, the gas has to be cooled. If the gas attains a final temperature of 157°C, find the initial temperature of the gas.
Fill in the blank with the correct word, from the words in option:
At -273°C the volume of a gas is theoretically ______.
A fixed volume of a gas occupies 760cm3 at 27°C and 70 cm of Hg. What will be its vol. at s.t.p.
The pressure on one mole of gas at s.t.p. is doubled and the temperature is raised to 546 K. What is the final volume of the gas ? [one mole of a gas occupies a volume of 22.4 litres at stp.]
