Home
Class 12
CHEMISTRY
Bond dissociation energy of O(2)(g) is x...

Bond dissociation energy of `O_(2)(g)` is `x k J mol^(-1)`. This means that

A

x kJ of energy is required to break one `O_2` molecule into atom

B

x kJ of energy is required to break 1 mole of O=O bonds in gaseous state into gaseous atoms

C

x kJ of energy is needed to convert `O_((g))` into `O_((g))^-`

D

x kJ of energy is needed to convert 1 g of `O_2` molecules into atoms

Text Solution

Verified by Experts

The correct Answer is:
B
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL THERMODYNAMICS AND ENERGETICS

    TARGET PUBLICATION|Exercise CRITICAL THINKING|95 Videos

  • CHEMICAL THERMODYNAMICS AND ENERGETICS

    TARGET PUBLICATION|Exercise COMPETITIVE THINKING|97 Videos

  • CHEMICAL KINETICS

    TARGET PUBLICATION|Exercise Evaluation test|13 Videos

  • CHEMISTRY IN EVERYDAY LIFE

    TARGET PUBLICATION|Exercise 7|3 Videos

Similar Questions

Explore conceptually related problems

The dissociation energy of CH_(4)(g) is 360 kcal mol^(-1) and that of C_(2)H_(6)(g) is 620 kcal mol^(-1) . The C-C bond energy

Ozone in the upper atmoshphere absorbs ultraviolet radiation which induces the following chemical reaction O_(3)(g)rightarrowO_(2)(g)+O(g) O_(2) produced in the above photochemical dissociation undergoes further dissociation into one normal oxygen atom (O) and more energetic oxygen atom O** . O_(2)(g) rightarrowO+O** (O**) has 1 eV more energy than(O) and normal dissociation energy of O_(2) is 480 kJ "mol"^(-1) . [1 eV/Photon =96 kJ "mol"^(-1) ] If dissociation of O_(3) into O_(2) and O requires 400kJ mol^(-1) and O_(2) produced in this reaction is further dissociated to O and O** then the total energy required to for the dissociation of O_(3) into O and O** is :

Ozone in the upper atmoshphere absorbs ultraviolet radiation which induces the following chemical reaction O_(3)(g)rightarrowO_(2)(g)+O(g) O_(2) produced in the above photochemical dissociation undergoes further dissociation into one normal oxygen atom (O) and more energetic oxygen atom O** . O_(2)(g) rightarrowO+O** (O**) has 1 eV more energy than(O) and normal dissociation energy of O_(2) is 480 kJ "mol"^(-1) . [1 eV/Photon =96 kJ "mol"^(-1) ] What is the maximum wavelength effective for the photochemical dissociation of O_(2) molecule

The average energy required to break a P-P bond in P_(4)(s) into gaseous atoms is 53.2 kcal mol^(-1) . The bond dissociation energy of H_(2)(g) is 104.2kcal mol^(-1) , Delta H_(f)^(0) of PH_(3)(g) from P_(4)(s) is 5.5 kcal mol^(-1) . The P-H bond energy in kcal mol^(-1) is [ Neglect presence of Van der Waals force in P_(4)(s) ]

The bond energy of H_(2) is 104.3 k.cal mol^(-1) . It means that

The bond energy of H_(2) is 104.3 kcal mol^(-1) . If means that :

The standard molar enthalpies of formation of H_(2)O(l) " and " H_(2)O_(2)(l) are -286 and -188 "kJ"//"mol", respectively. Molar enthalpies of vaporisation of H_(2)O(l) " and "H_(2)O_(2)(l) are 44 and 53 kJ respectively. The bond dissociation enthalpy of O_(2)(g) is 498 "kJ"//"mol" . calculate the bond dissociation enthalphy ("in" "kJ"//"mol" ) of O-O bond in H_(2)O_(2) , assuming that the bond dissociation ethalpy of O-H bond is same in both H_(2) " and " H_(2)O_(2) .

Bond dissociation energy of CH_(4) si 360 kJ/mol and C_(2)H_(6) has 620 kJ mol. Then bond dissociation energy of C-C bond is :-

Silanes are silicon hydrides of general formula Si_(n)Hn_(2n+2) and have several applications. From the data given below, the bond dissociation enthalpy of Si-Si bond ("in kJ mol"^(-1)) is Given: DeltaH of the reaction 2Si(s)+3H_(2)(g)rarrSi_(2)H_(6)(g)" is "80.3 kJ mol"^(-1) Bond dissociation enthalpy for H-H=436" kJ mol"^(-1) Bond dissociation enthalpy for Si-H=304" kJ mol"^(-1) Delta_(f)H[Si(g)]="450 kJ mol"^(-1)

TARGET PUBLICATION-CHEMICAL THERMODYNAMICS AND ENERGETICS -EVALUATION TEST
  1. Bond dissociation energy of O(2)(g) is x k J mol^(-1). This means that

    Text Solution

    |

  2. The enthalpy change for a reaction does not depend upon:

    Text Solution

    |

  3. The internal energy change when a system goes fromk state A to B is 40...

    Text Solution

    |

  4. Following gases have equal masses at the same temperature, pressure an...

    Text Solution

    |

  5. The standard enthalpy of formation (Delta(f)H^(@)) at 298K for methan...

    Text Solution

    |

  6. (Delta H - Delta U) for the formation of carbon monoxide (CO) from its...

    Text Solution

    |

  7. Identify the correct statement regarding a spontaneous process.

    Text Solution

    |

  8. Standard entropy of X(2) , Y(2) and XY(3) are 60, 40 and 50JK^(-1)mol...

    Text Solution

    |

  9. The heats of neutralisation of CH3 - COOH , H-COOH,HCN and H2 S are -1...

    Text Solution

    |

  10. The bond dissociation energy of gaseous H(2), Cl(2) and HCl are 104, 5...

    Text Solution

    |

  11. The difference between the heats of reaction at constant pressure and ...

    Text Solution

    |

  12. Given standard enthalpy of formation of CO(-110 "KJ mol"^(-1)) and CO(...

    Text Solution

    |

  13. H(2)(g)+1//2O(2)(g)=H(2)O(l) , Delta H(298 K)=-68.32 Kcal. Heat of vap...

    Text Solution

    |

  14. The heat change at constant volume for the decomposition of silver (I)...

    Text Solution

    |

  15. Which of the following value of DeltaH(f)^(@) represent that the produ...

    Text Solution

    |

  16. The enthalpy change (DeltaH) for the process N2H(4(g)) to 2N((g)) + 4H...

    Text Solution

    |

  17. For the two equations given below: H(2)(g)+1//2O(2)(g)toH(2)O(l)+x(1...

    Text Solution

    |

  18. For an endothermic reaction, where Delta H represents the enthalpy of ...

    Text Solution

    |

  19. The entropy chnge for a non-spontaneous reaction is 140 J/K.mole at 29...

    Text Solution

    |

  20. The entropy change for a certain non-spontaneous reaction is 150 J/K.m...

    Text Solution

    |

  21. C(2)H(4) +CI(2) rarr C(2)H(4)CI(2) DeltaH =- 270.6 kJ mol^(-1)K^(-1)...

    Text Solution

    |