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:
Give reasons for the following:
Mountaineers carry oxygen cylinders with them.
State the following:
Ice point in absolute temperature
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.
Taking the volume of hydrogen as calculated in Q.19, what change must be made in Kelvin (absolute) temperature to return the volume to 2500 cm3 (pressure remaining constant)?
State Charles's law.
At a given temperature the pressure of a gas reduces to 75% of its initial value and the volume increases by 40% of its initial value. Find this temperature if the initial temperature was -10°C.
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.]
The following question refers to one mole of chlorine gas.
What volume will it occupy at 273°C?
