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The standard enthalpy of formation (DfHº) 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 [2006]  
  • a)
    the first four ionization energies of carbon and electron gain enthalpy of hydrogen
  • b)
    the dissociation energy of hydrogen molecule, H2
  • c)
    the dissociation energy of H2 and enthalpy of sublimation of carbon
  • d)
    latent heat of vapourization of methane
Correct answer is option 'C'. Can you explain this answer?
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The standard enthalpy of formation (DfHº) at 298 K for methane, C...
The standard enthalpy of formation of CH4 is given by the equation : C(s) + 2H2(g) —​→ CH4(g)
Hence, dissociation energy of hydrogen and enthalpy of sublimation of carbon is required.
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The standard enthalpy of formation (DfHº) at 298 K for methane, C...
The standard enthalpy of formation (ΔfH) is the change in enthalpy that occurs when one mole of a substance is formed from its constituent elements in their standard states (usually at 25°C and 1 atm pressure). It is a measure of the energy released or absorbed during a chemical reaction.

The standard enthalpy of formation is typically reported in units of kilojoules per mole (kJ/mol). A positive value for ΔfH indicates that energy is absorbed during the formation of the substance, while a negative value indicates that energy is released.

The standard enthalpy of formation is useful in determining the overall energy change of a reaction, as it allows for the calculation of the enthalpy change (ΔH) for a reaction using the difference in the standard enthalpies of formation of the reactants and products.

The standard enthalpies of formation are generally tabulated and can be used to calculate the ΔH for a wide range of chemical reactions. These values are determined experimentally and are known with a high degree of accuracy for many common substances.
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Properties, whose values depend only on the concentration of solute particles in solution and not on the identity of the solute are called colligative properties. There may be change in number of moles of solute due to ionisation or association hence these properties are also affected. Number of moles of the product is related to degree of ionisation or association by vant Hoff factor ‘i’ given by i = [ 1 + (n – 1) α] for dissociationwhere n is the number of products (ions or molecules) obtained per mole of the reactant & i = for association.Where n is number of reactant particles associated to give 1 mole product.A dilute solution contains ‘t’ moles of solute X in 1 Kg of solvent with molal elevation constant Kb. The solute dimerises in the solution according to the following equation. The degree of association is α.Q.The equilibrium constant for the process can be expressed as

Properties, whose values depend only on the concentration of solute particles in solution and not on the identity of the solute are called colligative properties. There may be change in number of moles of solute due to ionisation or association hence these properties are also affected. Number of moles of the product is related to degree of ionisation or association by vant Hoff factor ‘i’ given by i = [ 1 + (n – 1) α] for dissociationwhere n is the number of products (ions or molecules) obtained per mole of the reactant & i = for association.Where n is number of reactant particles associated to give 1 mole product.A dilute solution contains ‘t’ moles of solute X in 1 Kg of solvent with molal elevation constant Kb. The solute dimerises in the solution according to the following equation. The degree of association is α.Q.The vant Hoff factor will be [ if we start with one mole of X ]

Properties, whose values depend only on the concentration of solute particles in solution and not on the identity of the solute are called colligative properties. There may be change in number of moles of solute due to ionisation or association hence these properties are also affected. Number of moles of the product is related to degree of ionisation or association by vant Hoff factor ‘i’ given by i = [ 1 + (n – 1) α] for dissociationwhere n is the number of products (ions or molecules) obtained per mole of the reactant & i = for association.Where n is number of reactant particles associated to give 1 mole product.A dilute solution contains ‘t’ moles of solute X in 1 Kg of solvent with molal elevation constant Kb. The solute dimerises in the solution according to the following equation. The degree of association is α.Q.The colligative properties observed will be

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The standard enthalpy of formation (DfHº) 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 [2006]a)the first four ionization energies of carbon and electron gain enthalpy of hydrogenb)the dissociation energy of hydrogen molecule, H2c)the dissociation energy of H2 and enthalpy of sublimation of carbond)latent heat of vapourization of methaneCorrect answer is option 'C'. Can you explain this answer?
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The standard enthalpy of formation (DfHº) 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 [2006]a)the first four ionization energies of carbon and electron gain enthalpy of hydrogenb)the dissociation energy of hydrogen molecule, H2c)the dissociation energy of H2 and enthalpy of sublimation of carbond)latent heat of vapourization of methaneCorrect answer is option 'C'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The standard enthalpy of formation (DfHº) 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 [2006]a)the first four ionization energies of carbon and electron gain enthalpy of hydrogenb)the dissociation energy of hydrogen molecule, H2c)the dissociation energy of H2 and enthalpy of sublimation of carbond)latent heat of vapourization of methaneCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The standard enthalpy of formation (DfHº) 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 [2006]a)the first four ionization energies of carbon and electron gain enthalpy of hydrogenb)the dissociation energy of hydrogen molecule, H2c)the dissociation energy of H2 and enthalpy of sublimation of carbond)latent heat of vapourization of methaneCorrect answer is option 'C'. Can you explain this answer?.
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