Advertisements
Advertisements
प्रश्न
Assuming temperature remaining constant calculate the pressure of the gas in the following:
The pressure of a gas having volume 1500 cm3 originally occupying 750 cc. at 5 ats. pressure.
Advertisements
उत्तर
V1 = 750 cc
P1 = 5 atm.
V2 = 1500 cc
P2 = ?
At constant temperature P1V1 = P2V2
∴ P2 = `("P"_1"V"_1)/"V"_2 = (5 xx 750)/(1500) = 5/2 = 2.5` atm.
APPEARS IN
संबंधित प्रश्न
State the law which is represented by the following graph:
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.
State Boyle’s Law.
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.]
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.
Fill in the blank with the correct word, from the words in option:
If the pressure of a fixed mass of a gas is kept constant and the temperature is increased, the volume correspondingly _______
According to Boyle’s law, the shape of the graph between pressure and reciprocal of volume is _______.
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?
