Home
Class 12
PHYSICS
A mass of diatomic gas(gamma=1.4) at a p...

A mass of diatomic gas`(gamma=1.4)` at a pressure of 2 atomphere is compressed adiabitically so that its temperature rises from `27^(@)C` to `927^(@)C`. The pressure of the gas in the final state is

A

256 atm

B

8 atm

C

26 atm

D

`68.7` atm

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    AAKASH INSTITUTE|Exercise ASSIGNMENT (SECTION -D) (Assertion - Reason Type Questions)|10 Videos
  • THERMODYNAMICS

    AAKASH INSTITUTE|Exercise ASSIGNMENT (SECTION -B) (Objective Type Questions)|23 Videos
  • THERMAL PROPERTIES OF MATTER

    AAKASH INSTITUTE|Exercise Assignment (Section-J) Akash Challengers Questions|7 Videos
  • UNITS AND MEASUREMENTS

    AAKASH INSTITUTE|Exercise ASSIGNMENT (SECTION - D)|15 Videos

Similar Questions

Explore conceptually related problems

One gm mol of a diatomic gas (gamma=1.4) is compressed adiabatically so that its temperature rises from 27^(@)C to 127^(@)C . The work done will be

One mole of an ideal gas (gamma=7//5) is adiabatically compressed so that its temperature rises from 27^(@)C to 35^(@)C the work done by the gas is (R=8.47J/mol-K)

A monatomic gas is compressed adiabatically to (1)/(4)^(th) of its original volume , the final pressure of gas in terms of initial pressure P 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)

An ideal gas at 17^(@)C has a pressure of 760 mm of Hg. The gas is compressed at constant temperature until its volume becomes halved. The final pressure of the gas will be –

One mole of an ideal gas with gamma=1.4 is adiabatically compressed so that its temperature rises from 27^(@)C to 34^(@)C . The change in the internal energy of the gas is (R=8.3J mol^(-10k^(-1)))

AAKASH INSTITUTE-THERMODYNAMICS-ASSIGNMENT (SECTION -C) (Previous Year Questions)
  1. One mole of an ideal gas goes from an initial state A to final state B...

    Text Solution

    |

  2. During an isothermal expansion, a confined ideal gas does -150 J of wo...

    Text Solution

    |

  3. A mass of diatomic gas(gamma=1.4) at a pressure of 2 atomphere is comp...

    Text Solution

    |

  4. If DeltaU and Delta W represent the increase in internal energy and wo...

    Text Solution

    |

  5. If C(p) and C(v) denote the specific heats (per unit mass of an ideal ...

    Text Solution

    |

  6. A monoatomic gas at pressure P(1) and volume V(1) is compressed adiaba...

    Text Solution

    |

  7. In thermodynamic processes which of the following statement is not tru...

    Text Solution

    |

  8. The internal energy change in a system that has absorbed 2 kcal of hea...

    Text Solution

    |

  9. If Q, E and W denote respectively the heat added, change in internal e...

    Text Solution

    |

  10. At 10^(@)C, the value of the density of a fixed mass of an ideal gas d...

    Text Solution

    |

  11. An engine has an efficiency of 1/6. When the temperature of sink is re...

    Text Solution

    |

  12. A Carnot engine whose sinl is at 300K has an efficiency of 40%. By how...

    Text Solution

    |

  13. The molar specific heat at constant pressure of an ideal gas is (7//2 ...

    Text Solution

    |

  14. Which of the following processes is reversible?

    Text Solution

    |

  15. An ideal gas heat engine operates in Carnot cycle between 227^(@)C and...

    Text Solution

    |

  16. A Carnot engine has efficiency 25%. It operates between reservoirs of ...

    Text Solution

    |

  17. In an adiabatic change, the pressure and temperature of a monoatomic g...

    Text Solution

    |

  18. An ideal Carnot's engine whose efficiency 40% receives heat of 500K. I...

    Text Solution

    |

  19. A diatomic gas initially at 18^(@) is compressed adiabatically to one-...

    Text Solution

    |

  20. An ideal gas undergoing adiabatic change has the following pressure-te...

    Text Solution

    |