A cylinder containing $H_{2} O (l)$ and $N_{2} (g)$ at $25^{o} C$ recorded a pressure of 500 mbar. The volume of cylinder is reduced to half by forcing the piston downward at the same temperature, the new pressure reading would be (aqueous tension $=$ $23$ mbar):

977

mbar

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

1000

mbar

No worries! We‘ve got your back. Try BYJU‘S free classes today!

1100

mbar

No worries! We‘ve got your back. Try BYJU‘S free classes today!

1023

mbar

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is D $977$ mbar
$P_{N_{2}} = 500 - 23 = 477$ mbar.

As the volume of the cylinder is reduced to half, the pressure is doubled.

$P_{N_{2}}$ after compression $2 \times 477 = 954$ mbar.

Total pressure $= 954 + 23 = 977$ mbar.

Suggest Corrections

Similar questions

Q. A cylinder with piston contains

N_{2}

and a small amount of liquid water at a temperature of

25^{o} C

(aqueous tension of water = 23.8 mm). The total pressure inside the cylinder is 600 mm of Hg, the piston in the cylinder is pushed downwards keeping temperature constant to reduced the volume to half of its initial value. What is the pressure of this condition?

Q. A certain mass of a gas taken in 1 litre cylinder exerts a pressure of 500

m m H g

at a certain temperature. If the gas is transferred to another cylinder where it exerts 20% more pressure, calculate the volume of the cylinder at the same temperature.

Q. A cylinder with a movable piston contains air under a pressure

P_{1}

and a soap bubble of radius 'r'. The pressure

P_{2}

to which the air should be compressed by slowly pushing the piston into the cylinder for the soap bubble to reduce its size by half will be (The surface tension is

σ

and the temperature T is maintained constant)

A cylinder with a movable piston contains 3 moles of hydrogen at standard temperature and pressure. The walls of the cylinder are made of heat insulator, and the piston is insulated by having a pile of sand on it/ by what factor does the pressure of the gas increase, if the gas is compressed to half it original volume?

Q. A cylinder contains a gas at temperature of

27^{0} C

and a pressure 1MPa. If the temperature of the gas is lowered to

23^{0} C

, the change in Pressure would be:

Join BYJU'S Learning Program

A cylinder containing H2O(l) and N2(g) at 25oC recorded a pressure of 500 mbar. The volume of cylinder is reduced to half by forcing the piston downward at the same temperature, the new pressure reading would be (aqueous tension = 23 mbar):

The correct option is D 977 mbarPN2=500−23=477 mbar.As the volume of the cylinder is reduced to half, the pressure is doubled.PN2 after compression 2×477=954 mbar.Total pressure =954+23=977 mbar.

A cylinder containing $H_{2} O (l)$ and $N_{2} (g)$ at $25^{o} C$ recorded a pressure of 500 mbar. The volume of cylinder is reduced to half by forcing the piston downward at the same temperature, the new pressure reading would be (aqueous tension $=$ $23$ mbar):

The correct option is D $977$ mbar
$P_{N_{2}} = 500 - 23 = 477$ mbar.

As the volume of the cylinder is reduced to half, the pressure is doubled.

$P_{N_{2}}$ after compression $2 \times 477 = 954$ mbar.

Total pressure $= 954 + 23 = 977$ mbar.