Home
Class 11
PHYSICS
Calculate the rise in temperature when a...

Calculate the rise in temperature when a gas, for which `gamma = 1.5` is compressed to 27 times its original pressure, assuming the initial temperature to be `27^(@)C`.

Text Solution

Verified by Experts

The correct Answer is:
`599.9^(@)C`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    SL ARORA|Exercise Exercise|342 Videos
  • THERMODYNAMICS

    SL ARORA|Exercise Problems from competitive examinations|22 Videos
  • Thermal Properties of Matter

    SL ARORA|Exercise Exercise|449 Videos
  • Units and Measurements

    SL ARORA|Exercise Exercise|499 Videos

Similar Questions

Explore conceptually related problems

Calculate the change in temperature when a gas ( gamma = 1.4) is suddenly allowed to expand to one hundredth of its original pressure, its original temperature being 37^@C .

A gas for which gamma=1.5 is suddenly compressed to 1//4 th of the initial volume. Then the ratio of the final to initial pressure is

An ideal gas at pressure of 1 atmosphere and temperature of 27^(@)C is compressed adiabatically until its pressure becomes 8 times the initial pressure, then the final temperature is (gamma=3//2)

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

Calculate the fall in temperature of helium initially at 15^(@)C , when it is suddenly expanded to 8 times its original volume (gamma=5//3) .

When the temperature of a gas in a metal is incrased from 27^(@)C to 87^(@)C the initial pressure of 2 atmospheres changes to

A gas is suddenly compressed to 1/4th of its original volume. Caculate the rise in temperature when original temperature is 27^(@)C. gamma= 1.5 .

A gas of gamma=1.4 and initial temperature 0^(@)C is suddenly compressed to 1//5th its original volume. Calculate the rise in temperature.

SL ARORA-THERMODYNAMICS-Problems for self practice
  1. A litre of hydrogen at 127^(@)C and 10^(6) dyne cm^(-2) pressure exp...

    Text Solution

    |

  2. Dry air at 15^@ C and 10 atm is suddenly released at atmospheric pres...

    Text Solution

    |

  3. Calculate the rise in temperature when a gas, for which gamma = 1.5 is...

    Text Solution

    |

  4. 1000 cm^(3) of argon at 27^(@)C is adiabatically compressed so that th...

    Text Solution

    |

  5. Calculate the work done if one mole of an ideal gas is compressed isot...

    Text Solution

    |

  6. One kilogram molecule of a gas at 400 K expands isothermally until its...

    Text Solution

    |

  7. Find the final value of a gram molecule of a gas after an isothermal e...

    Text Solution

    |

  8. One gram mole of an ideal gas at N.T.P is first expanded isothermally ...

    Text Solution

    |

  9. Calculate work done to compress isothermally 1g of hydrogen gas at N.T...

    Text Solution

    |

  10. Ten mole of hydrogen at N.T.P is compressed adiabatically so that it t...

    Text Solution

    |

  11. If 1 gram of oxygen at 760 mm pressure and 0^(@)C has its volume doubl...

    Text Solution

    |

  12. A sample of hydrogen of mass 6g is allowed to expand isothermally at 2...

    Text Solution

    |

  13. 50 g of oxygen at N.T.P. is compressed adiabatically to a pressure of ...

    Text Solution

    |

  14. Find the efficiency of a Carnot's engine working between 127^(@)C and ...

    Text Solution

    |

  15. A Carnot engine, whose temperature of the source is 400K receives 200 ...

    Text Solution

    |

  16. Calculate the efficiency of a Carnot engine operating between 450 K an...

    Text Solution

    |

  17. A Carnot engine whose low temperature reservoir is at 7^(@)C has an ef...

    Text Solution

    |

  18. Efficiency of a carnot engine is 0.4, when temp. of sink is 300K. What...

    Text Solution

    |

  19. A carnot engine absorbs 1000J of heat energy from a reservoir at 127^(...

    Text Solution

    |

  20. A reversible heat engine operates with an efficiency of 50 %. If durin...

    Text Solution

    |