Home
Class 11
CHEMISTRY
Consider the reaction: 2NO(g)+O(2)(g) ...

Consider the reaction:
`2NO(g)+O_(2)(g) rarr 2NO_(2)(g)`
Calculated the standard Gibbs energy change at `298K` and predict whether the reaction is spontaneous or not. `Delta_(f)G^(Theta) (NO) = 86.69 kJ mol^(-1), Delta_(f)G^(Theta) (NO_(2)) = 51.84 kJ mol^(-1)`.

Text Solution

Verified by Experts

The correct Answer is:
`-69.7 kJ` , spontaneous reaction.
For the reaction:
`2NO(g) + O_(2)(g) to 2NO_(2)(g)`
`DeltaG^(@) = 2Delta_(f)G^(@)(NO_(2)) - [2Delta_(f)G^(@)(NO) + Delta_(f)G^(@)(O_(2))]`
` 2 xx 51.84-2 xx 86.69 - 0`
` = 103.68 - 173.38`
` = -69.7 kJ mol^(-1)`.
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    MODERN PUBLICATION|Exercise Advanced Level Problems|15 Videos

  • THERMODYNAMICS

    MODERN PUBLICATION|Exercise Conceptual Questions -1|19 Videos

  • THERMODYNAMICS

    MODERN PUBLICATION|Exercise Unit Practice Test|12 Videos

  • STRUCTURE OF ATOM

    MODERN PUBLICATION|Exercise Unit Practice Test|13 Videos

Similar Questions

Explore conceptually related problems

Consider the reaction: 2NO(g)+O_(2)(g) rarr 2NO_(2)(g) Calculated the standard Gibbs energy change at 298K and predict whther the rection is spontaneous or not. Delta_(f)G^(Theta) (NO) = 86.69 kJ mol^(-1), Delta_(f)G^(Theta) (NO_(2)) = 51.84 kJ mol^(-1) .

Consider the reaction 2NO(g) + O_(2)(g) rarr 2NO_(2)(g) , Predict whether the reaction is spontaneous at 298 K. Delta_(f) G(NO) = 86.69k J//mol,Delta _(f) G ( NO_(2) = 51.84 kJ//mol

Will the reaction, I_(2)(s) +H_(2)S(g) rarr 2HI(g) +S(s) proceed spontaneously in the forward direction of 298K Delta_(f)G^(Theta)HI(g) = 1.8 kJ mol^(-1), Delta_(f)G^(Theta)H_(2)S(g) = 33.8 kJ mol^(-1) ?

Consider the reaction: 4NH_(3)(g) +5O_(2)(g) rarr 4NO(g) +6H_(2)O(l) DeltaG^(Theta) =- 1010.5 kJ Calculate Delta_(f)G^(Theta) [NO(g)] if Delta_(f)G^(Theta) (NH_(3)) = -16.6 kJ mol^(-1) and Delta_(f)G^(Theta) [H_(2)O(l)] =- 237.2 kJ mol^(-1) .

For the reaction, 2NOCl(g) hArr 2NO(g)+Cl_(2)(g) Calculate the standard equilibrium constant at 298 K . Given that the value of DeltaH^(ɵ) and DeltaS^(ɵ) of the reaction at 298 K are 77.2 kJ mol^(-1) and 122 J K^(-1) mol^(-1) .

Calculate the standard Gibbs free energy change from the free energies of formation data for the following reaction: C_(6)H_(6)(l) +(15)/(2)O_(2)(g) rarr 6CO_(2)(g) +3H_(2)O(g) Given that Delta_(f)G^(Theta) =[C_(6)H_(6)(l)] = 172.8 kJ mol^(-1) Delta_(f)G^(Theta)[CO_(2)(g)] =- 394.4 kJ mol^(-1) Delta_(f)G^(Theta) [H_(2)O(g)] =- 228.6 kJ mol^(-1)

Determine whether or not is possible for sodium to reduce aluminium oxide to aluminium at 298K . Also, calculate equilibrium constant for this reaction at 298K . Delta_(f)G^(Theta)AI_(2)O_(3)(s) =- 1582 kJ mol^(-1) Delta_(f)g^(Theta)Na_(2)O(s) =- 377.7 kJ mol^(-1)

The combustion of 1 mol of benzene takes place at 298 K and 1 atm . After combustion, CO_(2)(g) and H_(2)O(l) are produced and 3267.0 kJ of heat is librated. Calculate the standard entalpy of formation, Delta_(f)H^(Θ) of benzene Given: Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1) Delta_(f)H^(Θ)H_(2)O(l) = -285.83 kJ mol^(-1) .

MODERN PUBLICATION-THERMODYNAMICS-Practice Problems
  1. Calculate the Gibbs energy change on dissolving one mole of sodium chl...

    Text Solution

    |

  2. The value of DeltaH and DeltaS for two reactions are given below : R...

    Text Solution

    |

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

    Text Solution

    |

  4. For the reaction at 298 K 2A + B to C DeltaH = 40 kJ "mol"^(-1) a...

    Text Solution

    |

  5. Consider the reaction: 2NO(g)+O(2)(g) rarr 2NO(2)(g) Calculated th...

    Text Solution

    |

  6. Calculate the Delta(r)G^(@) for the reaction: C(6)H(12)O(6)(s) + 6O(...

    Text Solution

    |

  7. Calculate DeltaG^(@) for the reaction NO(g) iff 1/2 N(2)(g) + 1/2 O(...

    Text Solution

    |

  8. The equilibrium constant for the reaction CO(2)(g) +H(2)(g) hArr CO(...

    Text Solution

    |

  9. Calculated the equilibrium constant for the following reaction at 298K...

    Text Solution

    |

  10. The equilibrium constant for the reaction: CH(3)COOH(l) + C(2)H(5)OH...

    Text Solution

    |

  11. Calculate the entropy change for a reaction: XrarrY Given that Del...

    Text Solution

    |

  12. Calculate the equilibrium constant for the following reaction at 298K ...

    Text Solution

    |

  13. For the equilibrium reaction : 2H(2)(g) + O(2)(g) iff 2H(2)O(l) at 298...

    Text Solution

    |

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

    Text Solution

    |

  15. DeltaH^(Theta) and DeltaS^(Theta) for the reaction: Br(2)(l) +CI(2)(...

    Text Solution

    |

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

    Text Solution

    |

  17. Calculate Delta(r)G^(@) for the reaction : CO(g) + 1/2O(2)(g) to CO(2)...

    Text Solution

    |

  18. Calculate the change of entropy, Delta(r)S^(Theta) at 298K for the rea...

    Text Solution

    |

  19. Calculate the standard molar entropy chnage for the following reaction...

    Text Solution

    |

  20. Using Delta(f)H^(@) and S(m)^(@) calculate the standard Gibbs energy o...

    Text Solution

    |