Home
Class 11
CHEMISTRY
At 60^@C dinitrogen tetroxide is fifty p...

At `60^@C` dinitrogen tetroxide is fifty percent dissociated. Calculate the standard free energy change at this temperature and at one atmosphere. 

Text Solution

Verified by Experts

`N_2O_4 (9g) Leftrightarrow 2NO_2(b)`
If `N_2O_4` is 50% dissociated, the mole fraction of both the substances is given by
`x_(N_(2)O_(4))=(1-0.5)/(1+0.5), X_(NO_(2))=(2 xx 0.5)/(1+0.5)`
`P_(N2O4)=(0.5)/(1.5) xx 1 atm , P_(NO_(2))=(1)/(1.5) xx"1 atm"`
The equilibrium constant `K_P` is given by
`K_(p)=(p_(NO_(2))^2)/(P_(N_(2)O_(4))=(1.5)/((1.5)^2 (0.5))`
=1.33 atm
Since
`triangle_(r)G^@=-RT ln K_(p)`
`triangle_(r) G^@=-("8.314 JK"^(-1) mol^(-1)) xx (33K) xx (2.303) xx (0.1239)`
`=-763.8kJ mol"^(-1)`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    VIKRAM PUBLICATION ( ANDHRA PUBLICATION)|Exercise Very Short Answer Questions|37 Videos

  • THERMODYNAMICS

    VIKRAM PUBLICATION ( ANDHRA PUBLICATION)|Exercise Short Answer Questions|63 Videos

  • THE S-BLOCK ELEMENTS

    VIKRAM PUBLICATION ( ANDHRA PUBLICATION)|Exercise LONG ANSWER QUESTIONS |12 Videos

Similar Questions

Explore conceptually related problems

Calculate the standard Gibbs energy change for the redox reaction of Daniel cell .

The equilibrium constant of a reaction is 73. Calculate standard free energy change.

At 300 K, the equilibrium constant for a reaction is 10. the standard free energy change (in kJ mol^(-1) ) for the reaction is

For a spontaneous reaction, the free energy change must be negative. DeltaG=DeltaH-TDeltaS is the enthalpy change during the reaction. T is absolute temperature, and AS is the change in entropy during the reaction. Consider a reaction such as the formation ofan oxide . M+O_(2) MO Dloxygen is used wp in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids consequently gases have a higher entropy than liquids and solids, in this reaction (entropy or randomness) decreases, hence is negative. Thus, the temperature is raised the DeltaS becomes more negative. Since, TDeltaS is subtracted in the equation, then SG becomes less negative. Thus, the free energy changes increases with the increase in temperature. The free energy changes that occur when one mole of common reactant in this case dioxygen) is we may e plotted graphically against temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. Free energy change of Hg and Mg for the convertion to oxides the slope of DeltaG . T has been changed above the boiling points of the given metal because

For a spontaneous reaction, the free energy change must be negative. DeltaG=DeltaH-TDeltaS is the enthalpy change during the reaction. T is absolute temperature, and AS is the change in entropy during the reaction. Consider a reaction such as the formation ofan oxide . M+O_(2) MO Dloxygen is used wp in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids consequently gases have a higher entropy than liquids and solids, in this reaction (entropy or randomness) decreases, hence is negative. Thus, the temperature is raised the DeltaS becomes more negative. Since, TDeltaS is subtracted in the equation, then SG becomes less negative. Thus, the free energy changes increases with the increase in temperature. The free energy changes that occur when one mole of common reactant in this case dioxygen) is we may e plotted graphically against temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. Which of the following elements can be prepared by heating the oxide above 400^(@)C ?

For a spontaneous reaction, the free energy change must be negative. DeltaG=DeltaH-TDeltaS is the enthalpy change during the reaction. T is absolute temperature, and AS is the change in entropy during the reaction. Consider a reaction such as the formation ofan oxide . M+O_(2) MO Dloxygen is used wp in the course of this reaction. Gases have a more random structure (less ordered) than liquid or solids consequently gases have a higher entropy than liquids and solids, in this reaction (entropy or randomness) decreases, hence is negative. Thus, the temperature is raised the DeltaS becomes more negative. Since, TDeltaS is subtracted in the equation, then SG becomes less negative. Thus, the free energy changes increases with the increase in temperature. The free energy changes that occur when one mole of common reactant in this case dioxygen) is we may e plotted graphically against temperature for a number of reactions of metals to their oxides. The following plot is called an Ellingham diagram for metal oxide. Understanding of Ellingham diagram is extremely important for the efficient extraction of metals. As per the Ellingham diagram of oxides which of the following conclusion is true?

VIKRAM PUBLICATION ( ANDHRA PUBLICATION)-THERMODYNAMICS-Important Questions
  1. At 60^@C dinitrogen tetroxide is fifty percent dissociated. Calculate ...

    Text Solution

    |

  2. Define a system. Give an example.

    Text Solution

    |

  3. The wall is adiabatic and DeltaU=W(ad). What do you understand about t...

    Text Solution

    |

  4. Express the change in internal energy of a system when iii) w amount o...

    Text Solution

    |

  5. In isothermal free expansion of an ideal gas find the value of q and D...

    Text Solution

    |

  6. In isothermal irreversible change of ideal gas what is the value of q?

    Text Solution

    |

  7. In isothermal reversible change of an ideal gas, what is the value of ...

    Text Solution

    |

  8. For an adiabatic change of in an ideal gas what is the relationship be...

    Text Solution

    |

  9. State the first law of thermodynamics. Explain its mathematical notati...

    Text Solution

    |

  10. What are the sign conventions of the work done on the system and work ...

    Text Solution

    |

  11. No work is done on the system, but heat (q) is taken out from the syst...

    Text Solution

    |

  12. What are intensive and extensive properties?

    Text Solution

    |

  13. 1 g of graphite is burnt in a bomb calorimeter in excess of O(2) at 29...

    Text Solution

    |

  14. What is Delta(r)H for CH(4(g))+20(2(g))to CO(2(g))+2H(2)O(l) in terms ...

    Text Solution

    |

  15. Explain the relationship between Gibbs energy change and equilibrium c...

    Text Solution

    |

  16. State the third law of thermodynamics.

    Text Solution

    |

  17. What are open, closed and isolated systems ? Give one example for each...

    Text Solution

    |

  18. Define the state function and state variables. Give examples.

    Text Solution

    |

  19. "Internal energy is a state function." Explain.

    Text Solution

    |

  20. "Work is not a state function." Explain.

    Text Solution

    |

  21. Explain the state function 'enthalpy, H'. What is the relationship bet...

    Text Solution

    |