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The standard enthalpy of formation (ΔfHº) at 298 K for methane, CH4(g), is -74.8 kJ mol-1. The additional information required to determine the average energy for C - H bond formation would be -
[AIEEE 2006]
  • a)
    Latent heat of vaporization of methane
  • b)
    The first four ionization energies of carbon and electron gain enthalpy of hydrogen
  • c)
    The dissociation energy of hydrogen molecule H2
  • d)
    The dissociation energy of H2 and enthalpy of sublimation of carbon
Correct answer is option 'D'. Can you explain this answer?
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The standard enthalpy of formation (ΔfHº) at 298 K for meth...
The correct answer is option D
Carbon is found in the solid-state. The state of the substance affects the enthalpy change.
Hence, the correct option is A
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The standard enthalpy of formation (ΔfHº) at 298 K for meth...
Understanding the Formation of Methane
To calculate the average energy for C - H bond formation in methane, we need to consider the relevant thermodynamic values.
Key Thermodynamic Values Required
1. Dissociation Energy of H2:
- This value represents the energy required to break the H-H bond in molecular hydrogen. It is essential because methane contains four C-H bonds, and knowing how much energy is needed to produce hydrogen atoms from H2 is crucial for our calculations.
2. Enthalpy of Sublimation of Carbon:
- This value signifies the energy required to convert solid carbon (graphite) into gaseous carbon atoms. Since the formation of methane involves gaseous carbon atoms, this value is vital for determining the total energy changes involved in the formation of methane from its elements.
Why Other Options Are Not Sufficient
- Latent Heat of Vaporization of Methane:
- This property pertains to the phase change of methane from liquid to gas and does not directly influence the bond energies.
- First Four Ionization Energies of Carbon and Electron Gain Enthalpy of Hydrogen:
- While these values relate to the energy changes when forming ions, they do not directly contribute to the bond formation energies in methane.
Conclusion
The correct answer is option D because both the dissociation energy of H2 and the enthalpy of sublimation of carbon provide the necessary information to determine the energy changes involved in forming the C-H bonds in methane. By accounting for these energies, we can effectively calculate the average energy associated with C-H bond formation.
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The standard enthalpy of formation (ΔfHº) at 298 K for meth...
It's the e energy required to break a particular bond
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Attempt All sub parts from each question.Triple Point: The temperature of a substance remains constant during its change of state (phase chang e). A graph between the temperature T and the Pressure P of the substance is called a phase diagram or P-T diagram. The following figure shows the phase diagram of water and CO2. Such a phase diagram divides the P-T plane into a solid-region, the vapour-region and the liquid-region. The regions are separated by the curves such as sublimation curve (BO), fusion curve (AO) and vaporisation curve (CO). The points on sublimation curve represent states in which solid and vapour phases coexist. The point on the sublimation curve BO represent states in which the solid and vapour phases coexist. Points on the fusion curve AO represent states in which solid and liquid phase coexist. Points on the vaporisation curve CO represent states in which the liquid and vapour phases coexist. The temperature and pressure at which the fusion curve, the vaporisation curve and the sublimation curve meet and all the three phases of a substance coexist is called the triple point of the substance.Q. Triple point of CO2 is

Attempt All sub parts from each question.Triple Point: The temperature of a substance remains constant during its change of state (phase chang e). A graph between the temperature T and the Pressure P of the substance is called a phase diagram or P-T diagram. The following figure shows the phase diagram of water and CO2. Such a phase diagram divides the P-T plane into a solid-region, the vapour-region and the liquid-region. The regions are separated by the curves such as sublimation curve (BO), fusion curve (AO) and vaporisation curve (CO). The points on sublimation curve represent states in which solid and vapour phases coexist. The point on the sublimation curve BO represent states in which the solid and vapour phases coexist. Points on the fusion curve AO represent states in which solid and liquid phase coexist. Points on the vaporisation curve CO represent states in which the liquid and vapour phases coexist. The temperature and pressure at which the fusion curve, the vaporisation curve and the sublimation curve meet and all the three phases of a substance coexist is called the triple point of the substance.Q. Sublimation curve represents the coexistence of

Attempt All sub parts from each question.Triple Point: The temperature of a substance remains constant during its change of state (phase chang e). A graph between the temperature T and the Pressure P of the substance is called a phase diagram or P-T diagram. The following figure shows the phase diagram of water and CO2. Such a phase diagram divides the P-T plane into a solid-region, the vapour-region and the liquid-region. The regions are separated by the curves such as sublimation curve (BO), fusion curve (AO) and vaporisation curve (CO). The points on sublimation curve represent states in which solid and vapour phases coexist. The point on the sublimation curve BO represent states in which the solid and vapour phases coexist. Points on the fusion curve AO represent states in which solid and liquid phase coexist. Points on the vaporisation curve CO represent states in which the liquid and vapour phases coexist. The temperature and pressure at which the fusion curve, the vaporisation curve and the sublimation curve meet and all the three phases of a substance coexist is called the triple point of the substance.Q. During phase change of a substance

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The standard enthalpy of formation (ΔfHº) at 298 K for methane, CH4(g), is -74.8 kJ mol-1. The additional information required to determine the average energy for C - H bond formation would be -[AIEEE 2006]a)Latent heat of vaporization of methaneb)The first four ionization energies of carbon and electron gain enthalpy of hydrogenc)The dissociation energy of hydrogen molecule H2d)The dissociation energy of H2and enthalpy of sublimation of carbonCorrect answer is option 'D'. Can you explain this answer?
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The standard enthalpy of formation (ΔfHº) at 298 K for methane, CH4(g), is -74.8 kJ mol-1. The additional information required to determine the average energy for C - H bond formation would be -[AIEEE 2006]a)Latent heat of vaporization of methaneb)The first four ionization energies of carbon and electron gain enthalpy of hydrogenc)The dissociation energy of hydrogen molecule H2d)The dissociation energy of H2and enthalpy of sublimation of carbonCorrect answer is option 'D'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about The standard enthalpy of formation (ΔfHº) at 298 K for methane, CH4(g), is -74.8 kJ mol-1. The additional information required to determine the average energy for C - H bond formation would be -[AIEEE 2006]a)Latent heat of vaporization of methaneb)The first four ionization energies of carbon and electron gain enthalpy of hydrogenc)The dissociation energy of hydrogen molecule H2d)The dissociation energy of H2and enthalpy of sublimation of carbonCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The standard enthalpy of formation (ΔfHº) at 298 K for methane, CH4(g), is -74.8 kJ mol-1. The additional information required to determine the average energy for C - H bond formation would be -[AIEEE 2006]a)Latent heat of vaporization of methaneb)The first four ionization energies of carbon and electron gain enthalpy of hydrogenc)The dissociation energy of hydrogen molecule H2d)The dissociation energy of H2and enthalpy of sublimation of carbonCorrect answer is option 'D'. Can you explain this answer?.
Solutions for The standard enthalpy of formation (ΔfHº) at 298 K for methane, CH4(g), is -74.8 kJ mol-1. The additional information required to determine the average energy for C - H bond formation would be -[AIEEE 2006]a)Latent heat of vaporization of methaneb)The first four ionization energies of carbon and electron gain enthalpy of hydrogenc)The dissociation energy of hydrogen molecule H2d)The dissociation energy of H2and enthalpy of sublimation of carbonCorrect answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 11. Download more important topics, notes, lectures and mock test series for Class 11 Exam by signing up for free.
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