Home
Class 12
CHEMISTRY
What should be the value of final temper...

What should be the value of final temperature so that 1 L gas becomes 2.5 L at constant pressure if initial temperature was 300 K?

A

750 K

B

850 K

C

550 K

D

650 K

Text Solution

AI Generated Solution

Promotional Banner

Topper's Solved these Questions

Similar Questions

Explore conceptually related problems

What is the work done when 1 mole of a gas expands isothermally from 25 L to 250 L at a constant pressure of 1 atm and a temperature of 300 K ?

The change in the magnitude of the volume of an ideal gas when a small additional pressure DeltaP is applied at a constant temperature, is the same as the change when the temperature is reduced by a small quantity DeltaT at constant pressure. The initial temperature and pressure of the gas were 300 K and 2 atm. respectively. If |DeltaT|=C|DeltaP| then value of C in (K/atm) is __________.

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from intial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas in 300 K then total entropy change of system in the above process is: [R=0.0082L atm mol^(-1)K^(-1)=8.3J mol^(-1)K^(-1)]

One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is :

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R=0.082L atm mol^(-1) K^(-1)-=8.3J mol^(-1) K^(-1)]

Two moles of a certain ideal gas at 300K is cooled at constant volume so that the pressure is reduced to half the original value. Now the gas is heated at constant pressure so that its temperature becomes equal to the initial temperature. Find the total amount of heat absorbed by the gas in the process.

AAKASH INSTITUTE-TEST 2-EXERCISE
  1. What is the ratio of volume of 1 mole of nitrogen gas to 16 g oxygen g...

    Text Solution

    |

  2. Density of a gas 'd' is

    Text Solution

    |

  3. What should be the value of final temperature so that 1 L gas becomes ...

    Text Solution

    |

  4. Which of the following has dimensions of energy?

    Text Solution

    |

  5. The value of absolute temperature at which ice starts melting is

    Text Solution

    |

  6. At [300 K, delta G^0 (N2O5(g)) = -43 kJ mol^-1]. if at a particular in...

    Text Solution

    |

  7. Which among the following is a Lewis acid?

    Text Solution

    |

  8. Which one of the following salt is least soluble in water?

    Text Solution

    |

  9. If 100 ml of 0.1 M CH3COOH and 200 ml of 0.03 M NaOH solutions are mix...

    Text Solution

    |

  10. If enthalpy of hydrogenation of cyclohexene is [-x kJ mol^-1] and reso...

    Text Solution

    |

  11. Vapour pressure of a liquid depends on

    Text Solution

    |

  12. Heat of combustion of C(s), H2(g) and CH4 (g) respectively are -94, -6...

    Text Solution

    |

  13. If one mole of monoatomic ideal gas expanded from 2 atm to 0.5 atm at ...

    Text Solution

    |

  14. 2 moles monoatomic ideal gas is expanded isothermally and reversibly f...

    Text Solution

    |

  15. The internal energy change for the vapourisation of one mole water at ...

    Text Solution

    |

  16. At 273 K, ice and water are in equilibrium and enthalpy of fusion of i...

    Text Solution

    |

  17. In a container of 10 L volume, 20 g O2(g) and 2.8 g CO(g) are taken at...

    Text Solution

    |

  18. Compressibility factor (Z) for H2 (g) at STP is

    Text Solution

    |

  19. 0.48 g of a volatile substance upon vapourisation gives 112 ml vapours...

    Text Solution

    |

  20. Equal mass of oxygen and helium gases are mixed in a container at 27°C...

    Text Solution

    |