Home
Class 11
CHEMISTRY
The energy change due to the reaction ...

The energy change due to the reaction
`2Na(s) +CI_(2) (g) rarr2Na CI(s)` is `-826kJ`
The consumption of 1 mo1 of `CI_(2)` gas contracts the system by `22.4L` at 1 atm What is the enthalphy change of the reaction .

Text Solution

AI Generated Solution

To solve the problem, we need to calculate the enthalpy change (ΔH) for the given reaction. We are provided with the energy change (ΔU) and the work done (PΔV) due to the contraction of the system. Here’s a step-by-step solution: ### Step 1: Understand the given data - The energy change for the reaction is given as ΔU = -826 kJ. - The consumption of 1 mole of Cl₂ gas contracts the system by 22.4 L at 1 atm. ### Step 2: Calculate the work done (PΔV) The work done on the system can be calculated using the formula: ...
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercise|1 Videos

  • THERMODYNAMICS

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 6.1|26 Videos

  • STOICHIOMETRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|33 Videos

Similar Questions

Explore conceptually related problems

The enthalpy changes for two reactions are given by the equations: 2Cr(s) +(3)/(2)O_(2)(g) rarr Cr_(2)O_(3)(s), DeltaH^(Theta) =- 1130 kJ C(s) +(1)/(2)O_(2)(g)rarr CO(g), DeltaH^(Theta) =- 110 kJ What is the enthalpy change in kJ for the following reactions? 3C(s) +Cr_(2)O_(3)(s) rarr 2Cr(s) +3CO(g)

Calculate the entropy change at 298K for the reaction Br_(2)(l) +CI_(2)(g) rarr 2BrCI(g) DeltaH = 29.3 kJ at 298K . The entropies of Br_(2)(l), CI_(2)(g) , and BrCI(g) at the above temperature and 152.3, 223.0 and 239.7 J mol^(-1)K^(-1) respectively.

The enthalpy and entropy change for the reaction Br_(2)(l) + Cl_(2)(g) rightarrow 2BrCl(g) are 40 kJ mol^(-1) and 110 JK^(-1) mol ^(-1) repectively. The temperature at which the reaction will be in equilibrium is

The emf of the cell reaction Zn(s) +Cu^(2+) (aq) rarr Zn^(2+) (aQ) +Cu(s) is 1.1V . Calculate the free enegry change for the reaction. If the enthalpy of the reaction is -216.7 kJ mol^(-1) , calculate the entropy change for the reaction.

Use the bond energies in the table to estimate DeltaH for this reaction: CH_(2) = CH_(2) + Cl_(2) rarr CICH_(2) -CH_(2)CI

Calculate free energy change for the reaction: H_(2)(g) + CI_(2)(g) rarr 2H-CI(g) by using the bond enegry and entropy data. Bond energies of H-H, CI-CI , and H-CI bonds are 435, 240 , and 430 kJ mol^(-1) , respectively. Standard entropies of H_(2),CI_(2) , and HCI are 130.59, 222.95 , and 186.68 J K^(-1) mol^(-1) , respectively.

Consider the following reaction: 2NaN_(3)(s) rarr 2Na(s) +3N_(2)(g) The enthalpy change for this reaction at 1atm is equal to:

The value of K_(p) for the reaction at 27^(@)C Br_(2)(l)+CI_(2)(g)hArr2BrCI(g) is 1atm . At equilibrium in a closed container partial pressure of BrCI gas 0.1atm and at this temperature the vapour pressure of Br_(2)(l) is also 0.1 atm. Then what will be minimum moles of Br_(2)(l) to be added to 1 mole of CI_(2) , initially, to get above equilibrium stiuation,

DeltaH^(Theta) and DeltaS^(Theta) for the reaction: Br_(2)(l) +CI_(2)(g) hArr 2BrCI(g) at 298K are 29.3 kJ mol^(-1) and 104.1 J K^(-1) mol^(-1) , respectively. Calculate the equilibrium constant for the reaction.

The enthalpy and entropy change for the reaction: Br_(2)(l) + Cl_(2)(g) to 2BrCl(g) are 30 kJ mol^(-1) and 105 JK^(-1) mol^(-1) respectively. The temperature at which the reaction will be in equilibrium is:-

CENGAGE CHEMISTRY ENGLISH-THERMODYNAMICS-Archives (Subjective)
  1. The energy change due to the reaction 2Na(s) +CI(2) (g) rarr2Na CI(s...

    Text Solution

    |

  2. The enthalpies for the following reactions (DeltaH^(Theta)) at 25^(@)C...

    Text Solution

    |

  3. The standared enthalpies of formation at 298K for C C1(g), H(2)O(g), C...

    Text Solution

    |

  4. Given that: i. C(s) + O(2)(g) rarr CO(2)(g) , DeltaH =- 94.05 kcal ...

    Text Solution

    |

  5. The following statement is true only under some specific conditions. W...

    Text Solution

    |

  6. The bond dissociation energies of gaseous H(2),Cl(2), and HCl are 100,...

    Text Solution

    |

  7. The standard molar heat of formation of ethane, carbon dioxide and wat...

    Text Solution

    |

  8. An intimate mixture of ferric oxide and aluminium is used as solid fue...

    Text Solution

    |

  9. The enthalpy of combustion of H(2), cyclohexene (C(6)H(10)) and cycloh...

    Text Solution

    |

  10. CsOH +HCI rarr CsCI +H(2)O, DeltaH =- 13.4 kcal mol^(-1)……….(i) CsOH...

    Text Solution

    |

  11. Determine enthalpy change for, C(3)H(8(g))+H(2(g))rarr C(2)H(6(g))+C...

    Text Solution

    |

  12. Compute the heat of formation of liquid methyl alcohol in kilojoule pe...

    Text Solution

    |

  13. From the following data, calculate the enthalpy change for the combust...

    Text Solution

    |

  14. The standard heat of formation values of SF(6)(g), S(g), and F(g) are ...

    Text Solution

    |

  15. Show that the reaction CO(g) +(1//2)O(2)(g) rarr CO(2)(g) at 300K ...

    Text Solution

    |

  16. A sample of argon gas at 1atm pressure and 27^(@)C expands reversibly ...

    Text Solution

    |

  17. Determine the enthalpy of formation of B(2)H(6)(g) in kJ/mol of the fo...

    Text Solution

    |

  18. The standart potential of the following cell is 0.23 at 15^(@)C and 0....

    Text Solution

    |

  19. When 1pentyne (A) is treated with 4N alcoholic KOH at 175^(@)C, it is ...

    Text Solution

    |

  20. Two moles of a perfect gas undergo the following processes: a. A rev...

    Text Solution

    |

  21. C(v) values of He is always (3R)/(2) but C(v) values of H(2) is (3R)/(...

    Text Solution

    |