Home
Class 11
CHEMISTRY
Using van der Waals equation, calculate ...

Using van der Waals equation, calculate the constant `a` when `2 mol` of a gas confined in a `4 L` flasks exerts a pressure of `11.0 atm` at a temperature of `300 K`. The value of `b` is `0.05 L mol^(-1)`.

Text Solution

Verified by Experts

Subsituting the given data in the van der Waals equation of state
`(p+(n^(2)a)/(V^(2)))(V-nb)=nRT`
We get
`[11atm+((2mol)^(2)a)/((4L)^(2))][4L-(2mol)(0.05 Lmol^(-1))`
`=(2 mol)(0.082 L atm K^(-1) mol^(-1))(300 K)`
or `(11 atm+a mol^(2) L^(-2)//4)( 4L-0.1 L)=49.2 L atm`
or `a=4((49.2)/(3.9)-11)L^(2)mol^(-2)atm`
`=4(12.615-11)L^(2) atm mol^(-2)`
`=6.46 L^(2)atm mol^(-1)`
Promotional Banner

Topper's Solved these Questions

  • STATES OF MATTER

    CENGAGE CHEMISTRY|Exercise Exercises|21 Videos

  • STATES OF MATTER

    CENGAGE CHEMISTRY|Exercise Exercises (Linked Comprehensive)|48 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

van der Waal's equation for calculating the pressure of a non ideal gas is (P+(an^(2))/(V^(2)))(V-nb)=nRT van der Waal's suggested that the pressure exerted by an ideal gas , P_("ideal") , is related to the experiventally measured pressure, P_("ideal") by the equation P_("ideal")=underset("observed pressure")(underset(uarr)(P_("real")))+underset("currection term")(underset(uarr)((an^(2))/(V^(2)))) Constant 'a' is measure of intermolecular interaction between gaseous molecules that gives rise to nonideal behavior. It depends upon how frequently any two molecules approach each other closely. Another correction concerns the volume occupied by the gas molecules. In the ideal gas equation, V represents the volume of the container. However, each molecule does occupy a finite, although small, intrinsic volume, so the effective volume of the gas vecomes (V-nb), where n is the number of moles of the gas and b is a constant. The term nb represents the volume occupied by gas particles present in n moles of the gas . Having taken into account the corrections for pressure and volume, we can rewrite the ideal gas equation as follows : underset("corrected pressure")((P+(an^(2))/(V^(2))))underset("corrected volume")((V-nb))=nRT Using van der Waals' equation, find the constant 'a' (in atm L^(2)mol^(-2) ) when two moles of a gas confined in 4 L flask exerts a pressure of 11.0 atmospheres at a temperature of 300 K. The value of b is 0.05 L mol^(-1) .(R = 0.082 atm.L/K mol)

Two moles of a real gas confined in a 5 L flask exerts a pressure 9.1 atm at a temperature of 27^(@)C . Calculate the value of 'a' given the value of b is "0.052 L mol"^(-1) .

The van der Waals equation for one mol of CO_(2) gas at low pressure will be

Calculate the temperature of the gas if it obeys van der Waal's equation from the following data. A flask of 2.5 litre contains 10 mole of a gas under 50 atm. Given a = 5.46 atm "litre"^(2) mol^(-2) " and " b = 0.031 " litre " mol^(-1)

(i) Prove that osmotic pressure is a colligative property. (ii) Calculate the molar of urea solution if it exerts an osmotic pressure of 2.45 atmosphere at 300K. (R = 0.0821 L atm. mol^(-1) K^(-1) ).

For a real gas critical pressure is 75 atm and van der Waal's constant 'b' is 40 millilitres per mole. If critical temperature of gas is TK. Calculate value of ((T)/(100)).["Use" R=0.08"L atm mol"^(-1)K^(-1)] .

One mole of a certain gas is contained in a vessel of volume V = 0.250 1 . At a temperature T_1 = 300 K the gas pressure is p_1 = 90 atm , and at a temperature T_2 = 350 K the pressure is p_2 = 110 atm . Find the Van der Walls parameters for this gas

Calculate the temperature of 2 moles of sulphur dioxide gas contained in a 5 L vessel at 10 bar pressure. Given that for SO_(2) gas, van der Waals constants are : a=6.7 bar L^(2) mol^(-2) and b=0.0564 L mol^(-1) .

CENGAGE CHEMISTRY-STATES OF MATTER-Exercises (Ture False)
  1. Using van der Waals equation, calculate the constant a when 2 mol of a...

    Text Solution

    |

  2. In the van der Waals equation (P + (n^(2)a)/(V^(2)))(V - nb) = nRT ...

    Text Solution

    |

  3. Kinetic energy of a molecule is zero at 0^(@)C

    Text Solution

    |

  4. A gas in a closed container will exert much higher pressure due to gra...

    Text Solution

    |

  5. The graph between PV vs P at constant temperature is linear parallel t...

    Text Solution

    |

  6. Real gases show deviation from ideal behaviour at low temperature and ...

    Text Solution

    |

  7. In the microscopic model of the gas, all the moleculer are supposed to...

    Text Solution

    |

  8. For real gases, at high temperature Z = 0 small value of a means gas...

    Text Solution

    |

  9. Small value of a means, gas can be easily liqueifed.

    Text Solution

    |

  10. Rate of diffusion is directly proportional to the square root of molec...

    Text Solution

    |

  11. For ideal gases, Z = 1 at all temperature and pressure.

    Text Solution

    |

  12. According to charles's law,

    Text Solution

    |

  13. The pressure of moist gas is higher than pressure of dry gas.

    Text Solution

    |

  14. Gases do not occupy volume and do not have force of attraction.

    Text Solution

    |

  15. The van der Waal equation of gas is (P + (n^(2)a)/(V^(2))) (V - nb)...

    Text Solution

    |

  16. Surface tension and surface energy have different dimensions.

    Text Solution

    |

  17. The plot of PV vs P at particular temperature is called isovbar.

    Text Solution

    |

  18. Equal volume of all gases always contains equal number of moles.

    Text Solution

    |

  19. A gas with a = 0 cannot be liquified.

    Text Solution

    |

  20. The van der waals constants have same values for all the gases.

    Text Solution

    |

  21. All the molecules in a given sample of gas move with same speed.

    Text Solution

    |