How much energy, in kilojoules, are released or absorbed from the reaction of 1 mole of #N_2#, nitrogen, with 3 moles of molecular hydrogen, #H_2#, to form 2 moles of ammonia, #NH_3#?

Answer 1

Wyatt Atkins

So you want the enthalpy associated with the reaction....

#N_2(g) +3H_2(g) rarr 2NH_3(g)+Delta#

Thus, we obtained.....

#DeltaH_"rxn"^@=2xxDeltaH_f^@NH_3(g)=2*molxx-46*kJ*mol^-1=-92*kJ.#

Of course #DeltaH_f^@NH_3(g)# is the enthalpy associated with ONE MOLE of ammonia....

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Answer 2

Luna Chen

The reaction you're referring to is the formation of ammonia (NH3) from nitrogen (N2) and hydrogen (H2), commonly known as the Haber process. This reaction is:

N2(g) + 3H2(g) → 2NH3(g)

The standard enthalpy change for this reaction, ΔH°, is -92.22 kJ/mol. Therefore, when 1 mole of N2 reacts with 3 moles of H2 to form 2 moles of NH3, the energy released is -92.22 kJ/mol.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.