Home
Class 12
CHEMISTRY
An ideal gas (gamma = (5)/(3)) is adiaba...

An ideal gas `(gamma = (5)/(3))` is adiabatically compressed from `640 cm^(3)` to `80cm^(3)`. If the initial pressure is `P` then find the final pressure?

Text Solution

Verified by Experts

Process is adiabatic `rArrP(640)^(gamma) rArrP_(1)=8^(5//3)=32P`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise F-7|1 Videos

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise F-8|1 Videos

  • THERMODYNAMICS

    RESONANCE ENGLISH|Exercise F-5|1 Videos

  • TEST SERIES

    RESONANCE ENGLISH|Exercise CHEMISTRY|50 Videos

Similar Questions

Explore conceptually related problems

A given sample of an ideal gas (gamma = 1.5 ) is compressed adiabatically from a volume of 150 cm ^(3) to 50 cm ^(3) . The initial pressure and the initial temperature are 150 kpa and 300K . Find (a) the number of moles of the gas in the sample, (b) the molar heat capacity at constant volume, (c) the final pressure and temperature, (d) the work done by the gas in the process and (e) the change in internal energy of the gas .

A sample of gas (gamma = 1.5) is taken through an adiabatic process in which the volume is compressed from 1600 cm^(3) to 400 cm^(3) . If the initial pressure is 150 kPa , (a) what is the final pressure and (b) how much work is done by the gas in the process?

Knowledge Check

  • For a gas gamma = 5//3 and 800 c.c, of this gas is suddenly compressed to 100 c.c. If the intial pressure is P, then final pressure will be

    A
    P/32
    B
    `(24//5)P`
    C
    0.83333333333333
    D
    32 P

    • Similar Questions

    Explore conceptually related problems

    The volume of an ideal gas (gamma = 1.5 ) is changed adiabatically from 4.00 liters to 3.00 liters . Find the ratio of (a) the final pressure to the initial pressure and (b) the final temperature to the initial temperature.

    An ideal gas (gamma=3//2) is compressed adiabatically form volume 400cm^(3) to 100cm^(3) . The initial pressure and temperature are 100 kPa and 400K . Find (a) the number of moles of the gas (b) the molar heat capacity at constant pressure, (c ) the final pressure and temperature, (d) the work done by the gas in the process and (e) the change in internal energy of the gas. (R = (25)/(3)J//mol-k)

    400 c c volume of gas having gamma=5/2 is suddenly compressed to 100 c c . If the initial pressure is P , the final pressure will be

    Air contained in a cylinder at 20.0^(@)C is compressed froma n initial pressure of 1.00 atm, and volume of 700 cm^(3) to a volume of 70.0cm^(3) . If the final pressure is 15.0 atm then what is the final temperature?

    300K a gas (gamma = 5//3) is compressed adiabatically so that its pressure becomes 1//8 of the original pressure. The final temperature of the gas is :

    An ideal gas initially at pressure 1 bar is being compressed from 30m^(3) to 10m^(3) volume and its temperature decreases from 320 K to 280 K then find final pressure of gas.

    A sample of ideal gas undergoes isothermal expansion in a reversible manner from volume V_(1) to volume V_(2) . The initial pressure is P_(1) and the final pressure is P_(2) . The same sample is then allowed to undergoes reversible expansion under adiabatic conditions from volume V_(1) to V_(2) . The initial pressure being same but final pressure is P_(3) . Which relation is correct (gamma = (C_(P))/(C_(V))) ?

    Home
    Profile