Home
Class 11
PHYSICS
1 mole of H(2) gas is contained in box o...

1 mole of `H_(2)` gas is contained in box of volume `V= 1.00 m^(3) at T = 300 K`. The gas is heated to a temperature of T = 3000 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

A

same as the pressure initially

B

2 times the pressure initially

C

10 times the pressure initially

D

20 times the pressure initially

Text Solution

Verified by Experts

The correct Answer is:
D
Accoding to gas equation,
PV= nRT
`or (P_(2)V_(2))/(T_(2))=(P_(1)V_(1))/(T_(1))or (P_(2))/(P_(1))=(V_(1))/(V_(2)).(T_(2))/(T_(1))`
Here, `T_(2)=3000 K,T_(1)=300K`
Since `H_(2)` splits into hydrogen atoms, therefore volume become half i.e., `V_(2)1/2V_(1)`
`(P_(2))/(P_(1))=(V_(1))/(1/2V_(1))xx(3000)/(300)or (P_(2))/(P_(1))=20`
Promotional Banner

Topper's Solved these Questions

  • KINETIC THEORY

    NCERT FINGERTIPS|Exercise Assertion And Reason|10 Videos

  • KINETIC THEORY

    NCERT FINGERTIPS|Exercise Higher Order Thinking Skills|10 Videos

  • GRAVITATION

    NCERT FINGERTIPS|Exercise Assertion And Reason|15 Videos

  • LAWS OF MOTION

    NCERT FINGERTIPS|Exercise Assertion And Reason|15 Videos

Similar Questions

Explore conceptually related problems

1 mole of H_(2) gas in contained in a box of volume V 1.00 m^(3) at T =300 K. The gas is heated to a temperature of T= 3000K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

One mole of a certain gas is contained in a vessel of volume V = 0.250 1 . At a temperature T_1 = 300 K the gas pressure is p_1 = 90 atm , and at a temperature T_2 = 350 K the pressure is p_2 = 110 atm . Find the Van der Walls parameters for this gas

An ideal gas is expanded adiabatically at an initial temperature of 300 K so that its volume is doubled. The final temperature of the hydrogen gas is lambda=1.40)

Initial volume of a gas is 1 L at temperature 100 K . What is the volume of a gas at 300 K .

One mole of oxygen is expanded from a volume V_1 = 1.00 1 to V_2 = 5.0 1 at a constant temperature T = 280 K . Calculate : (i) the increment of te internal energy of the gas : (b) the amount of the absorbed heat. The gas is assumed to be a Van der Walls gas.

An ideal gas is present in an open vessel at 27^(@)C . If this gas is heated upto TK temperature so that (2)/(3) of final moles of gas are escaped out, then calculate final temperature T.

In a process V prop T^(2) , temperature of 2 moles of a gas is increased by 200K. Work done by the gas in this process will be

At pressure P and absolute temperature T a mass M of an ideal gas fills a closed container of volume V. An additional mass 2M of the same gas is added into the container and the volume is then reduced to V/3 and the temperature to T/3 . The pressure of the gas will now be: