Home
Class 11
CHEMISTRY
Calculate the equilibrium constant for t...

Calculate the equilibrium constant for the reaction : `NO(g) + 1/2 O_(2)(g) iff NO_(2)(g)`
Given, `Delta_(f)H^(@) at 298K : NO(g) = 90.4 kJ "mol"^(-1), NO_(2)(g) = 33.8 kJ "mol"^(-1)` and `DeltaS^(@)` at `298 K = -70.8 J K^(-1) "mol"^(-1)`, `R = 8.31 J K^(-1) "mol"^(-1)`.

Text Solution

Verified by Experts

The correct Answer is:
`1.679xx 10^(6)`
`Delta_(r)H^(@) = Delta_(f) H^(@) ( NO_(2)) -[Delta_(f) H^(@) (NO)+(1)/(2) Delta_(f) H^(@) (O_(2))]= 33.8 -[90.4 + 0] = - 56.6kJ mol^(-1)`
`= - 56600 J mol^(-1) - 298 K ( - 70.8 JK^(-1) mol^(-1)) = - 35501.6 J mol^(-1)`
`:. - 35501.6 = - 2.303 xx 8.31 xx298 log K ` or `log K = 6.2250` or `K = 1.679 xx 10^(6)`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    PRADEEP|Exercise CURIOSITY QUESTIONS|4 Videos

  • THERMODYNAMICS

    PRADEEP|Exercise ADVANCED PROBLEMS (FOR COMPETITIONS)|20 Videos

  • THERMODYNAMICS

    PRADEEP|Exercise PROBLEMS FOR PRACTICE|14 Videos

  • STRUCTURE OF ATOM

    PRADEEP|Exercise Competition Focus (JEE (Main and Advanced)/Medical Entrance (IX. Assertion And Reason Type Questions (Type II))|12 Videos

Similar Questions

Explore conceptually related problems

Calculate the equilibrium constant for the reaction : NO(g) + 1/2 O_(2)(g) iff NO_(2)(g) Given, Delta_(f)H^(@) at 298 K : NO(g) = 90.4 kJ "mol"^(-1), NO_(2)(g) = 33.8 kJ "mol"^(-1) and DeltaS^(@) at 298 K = -70.8 J K^(-1) "mol"^(-1)

Calculated the equilibrium constant for the following reaction at 298K : 2H_(2)O(l) rarr 2H_(2)(g) +O_(2)(g) Delta_(f)G^(Theta) (H_(2)O) =- 237.2 kJ mol^(-1),R = 8.314 J mol^(-1) K^(-1)

Calculate equilibrium constant for the reaction: 2SO_(2)(g) +O_(2)(g) hArr 2SO_(3)(g) at 25^(@)C Given: Delta_(f)G^(Theta) SO_(3)(g) = - 371.1 kJ mol^(-1) , Delta_(f)G^(Theta)SO_(2)(g) =- 300.2 kJ mol^(-1) and R = 8.31 J K^(-1) mol^(-1)

Calculate the equilibrium constant, K for the following reaction at 400K? 2NOCl_((g))iff2NO_((g))+Cl_(2(g)) Given that Delta_(r)H^(0)=80.0KJmol^(-1) and Delta_(r)S^(0)=120JK^(-1)mol^(-1) at 400 K.

Calculate the standard free energy change for the reaction : H_(2)(g) + I_(2)(g) to 2HI(g) DeltaH^(@) = 51.9 kJ "mol"^(-1) Given : S^(@)(H_(2)) = 130.6 J K^(-1) "mol"^(-1) S^(@)(I_(2)) = 116.7 J K^(-1) "mol"^(-1) and S^(@)(HI) = 206.3 J K^(-1) "mol"^(-1) .

Calculate the equilibrium constant for the following reaction at 298K and 1 atmospheric pressure: C(graphite) +H_(2)O(l) rarr CO(g) +H_(2)(g) Given Delta_(f)H^(Theta) at 298 K for H_(2)O(l) =- 286.0 kJ mol^(-1) for CO(g) =- 110.5 kJ mol^(-1) DeltaS^(Theta) at 298K for the reaction = 252.6 J K^(-1) mol^(-1)

What is the equilibrium constant K_(c) for the following reaction at 400K ? 2NOCI(g) hArr 2NO(g) +CI_(2)(g) DeltaH^(Theta) = 77.2 kJ mol^(-1) and DeltaS^(Theta) = 122 J K^(-1) mol^(-1) at 400K .

PRADEEP-THERMODYNAMICS-PROBLEM FOR PRACTICE
  1. Calculate the free energy change in dissolving one mole of sodium chlo...

    Text Solution

    |

  2. The following data is known about the melting of KCl: DeltaH=7.25kJ"...

    Text Solution

    |

  3. The free enegry changes for the two reactions given below are a. SO(...

    Text Solution

    |

  4. At what temperature does the reduction of lead oxide to lead by carbon...

    Text Solution

    |

  5. For the reaction : 2NO(g) + O(2)(g) rarr 2NO(2)(g), the enthalpy and e...

    Text Solution

    |

  6. For a hypothetical reaction , X rarr Y , the enthalpy and entropy chan...

    Text Solution

    |

  7. The standard free energy change for a reaction is -212.3 kJ mol^(-1). ...

    Text Solution

    |

  8. For the reaction N(2)(g) + 3H(2)(g) rarr 2NH(2)(g), DeltaH = - 95.4 K...

    Text Solution

    |

  9. A chemist claims that the following reaction is feasible at 298 K SF...

    Text Solution

    |

  10. Calculate the standard free energy change for the reaction : Fe(2)O(3)...

    Text Solution

    |

  11. A chemist claims that the following reaction is feasible at 298 K SF...

    Text Solution

    |

  12. The value of K(p) for the water gas reaction, CO +H(2)O hArr CO(2) +H(...

    Text Solution

    |

  13. Calculate the equilibrium constant for the reaction : NO(g) + 1/2 O(2)...

    Text Solution

    |

  14. Calculate the standard entropy change for a reaction X harr Y, If the ...

    Text Solution

    |

  15. Using the following data, calculate the value of equilibrium constant ...

    Text Solution

    |

  16. Find out the value of equilibrium constant for the following reaction ...

    Text Solution

    |

  17. Calculate the standard free energy change for the reaction : H(2)(g)...

    Text Solution

    |

  18. Calculate the standard entropy change for the following reaction : ...

    Text Solution

    |

  19. Calculate the standard Gibbs energy change for the formation of propan...

    Text Solution

    |

  20. For oxidation of iron. 4Fe(s)+3O(2)(g)rarr2Fe(2)O(3)(s) entropy ch...

    Text Solution

    |