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What is the enthalpy of formation, ∆Hf, of hydrogen
iodide at 298 K? (Note: The bond energies of H2(g), I2(g), and HI(g) at 298 K are 436 kJ/mol, 151 kJ/mol, and 298 kJ/mol, respectively.)
Okay so the relevant equation is H2+I2-->2HI. Now I got this wrong because I calculated the total energy released, which is something like -9 kJ. When they say enthalpy of formation, are they just talking about ONE MOLE of product formed? So I shouldve divided my answer in two?
So do we need to make a distinction between the total heat released/heat of reaction AND heat of formation? One is extrinsic and the latter is intrinsic (without regard to number of moles)?
iodide at 298 K? (Note: The bond energies of H2(g), I2(g), and HI(g) at 298 K are 436 kJ/mol, 151 kJ/mol, and 298 kJ/mol, respectively.)
Okay so the relevant equation is H2+I2-->2HI. Now I got this wrong because I calculated the total energy released, which is something like -9 kJ. When they say enthalpy of formation, are they just talking about ONE MOLE of product formed? So I shouldve divided my answer in two?
So do we need to make a distinction between the total heat released/heat of reaction AND heat of formation? One is extrinsic and the latter is intrinsic (without regard to number of moles)?