Home
Class 11
CHEMISTRY
300 L of ammonia gas at 20^(@)C and 20 a...

300 L of ammonia gas at `20^(@)C` and 20 atm pressure is allowed to expand in a space of 600 L capacity and to a pressure of 1 atm. Calculate the drop in temperature.

Text Solution

Verified by Experts

`(P_(1)V_(1))/(T_(1))=(P_(2)V_(2))/(T_(2))=(20" atm"xx300L)/(293K)=(1" atm"xx600L)/(T_(2))`
or `T_(2)=29.3K`
`therefore` drop in temperature `=293-29.3=263.7K`
Promotional Banner

Topper's Solved these Questions

  • STATES OF MATTER

    CENGAGE CHEMISTRY|Exercise Ex 5.3|16 Videos

  • STATES OF MATTER

    CENGAGE CHEMISTRY|Exercise Ex 5.4|32 Videos

  • STATES OF MATTER

    CENGAGE CHEMISTRY|Exercise Ex 5.1|15 Videos

  • SOME BASIC CONCEPTS AND MOLE CONCEPT

    CENGAGE CHEMISTRY|Exercise Archives Subjective|11 Videos

  • STOICHIOMETRY

    CENGAGE CHEMISTRY|Exercise Archives Subjective|33 Videos

Similar Questions

Explore conceptually related problems

30 litre of ammonia gas at 30^@C and 40 atm pressure is allowed to expand in a space of 40 litre capacity and pressure becomes 20 atm. Calculate the drop in temperature.

An ideal gas is allowed to expand from 1 L to 10 L against a constant external pressure of 1 bar. Calculate the work done inkJ.

2.8 g of N_(2) gas at 300 K and 20 atm was allowed to expand isothermally against a constant external pressure of 1 atm. Calculate W for the gas.

A gas expands by 0.5L against a constant pressure of 1 atm . Calculate the work done in joule and calorie.

200 cm^(2) of a ga at 800 mm pressure is allowed to expand till the pressure is 0.9 atm keeping ath temperature constant. Calculate the volume of the gas.

2.8g of N_(2) gas at 300K and 20atm was allowed to expand isothermally against a constant external pressure of 1atm . Calculate DeltaU, q, and W for the gas.

A gas at 27°C and pressure 30 atm is allowed to expand to 1 atm pressure and volume 15 times larger. The final temperature of the gas is

10 itres of monoatomic gas at 0^(@) C and 10 atm pressure is suddenly released to 1 atm pressure and the gas expands adibatically against the constant pressure. The final temperature and the volume of the gas respectively are :

A quantity of an ideal gas at 20^(@)C reversibly expands against a constant pressure of 2.0 atm from 1.0 L to 2.0 L. Calculate the work done

CENGAGE CHEMISTRY-STATES OF MATTER-Ex 5.2
  1. Assuming ideal behaviour, calculate Boyle's law constant for each of t...

    Text Solution

    |

  2. A sample of gas is taken in a closed vessel at 20^(@)C. The gas is hea...

    Text Solution

    |

  3. What volume of O(2) at 2.00 atm pressure and 27^(@)C is requried to bu...

    Text Solution

    |

  4. The mass of 525 cm^(3) of a gaseous compound at 28^(@)C and 730 torr w...

    Text Solution

    |

  5. The temperature and pressure in Chnadigarh are 35^(@)C and 740 mm, res...

    Text Solution

    |

  6. Two flasks A and B have equal volume. Flask A contains hydrogen at 300...

    Text Solution

    |

  7. 2.9 g of a gas at 90^(@)C occupie the same volume as 0.184 g of H(2) a...

    Text Solution

    |

  8. Calculate the pressure of 4.0 mol of a gas occupying 5 dm^(3) at 3.32 ...

    Text Solution

    |

  9. Calculate the pressure exerted by 56 g of an ideal gas (with molar mas...

    Text Solution

    |

  10. An air bubble has a radius of 0.50 cm at the bottom of a water tank wh...

    Text Solution

    |

  11. A gas cylinder having a volume of 25.0 L contains a mixtue of butane C...

    Text Solution

    |

  12. 600 mL of nitrogen at 30 K is cooled to 5 K at the same pressure. Cal...

    Text Solution

    |

  13. 300 L of ammonia gas at 20^(@)C and 20 atm pressure is allowed to expa...

    Text Solution

    |

  14. A 1 L flask cantaing vapours of methyl alcohol (molar mass 32) at a pr...

    Text Solution

    |

  15. Temperature at the foot of a mountian is 30^(@)C and pressure is 760 m...

    Text Solution

    |

  16. A large flask fitted with a stopcock is evacuated and weighted. Its ma...

    Text Solution

    |