Question

N2O4(g) + 4H2(g) → N2(g) + 4H2O(g), solve using standard enthalpies of formation

Answer 1

The standard enthalpy of formation (Δ$H_f$) is a measure of the energy released or consumed when one mole of a substance is created under standard conditions from its pure elements.

Standard enthalpies (Δ$H_f$) of formation for given reaction is 978.3 kJ

What is Standard enthalpies of formation?

The standard enthalpy of formation is defined as the enthalpy change when one mole of a substance in the standard state (1 atm of pressure and 298.15 K) is formed from its pure elements under the same conditions.

Given reaction ;

$N_2O_4(g) + 4H_2 (g) - > N_2(g) + 4H_2O(g)$

To Find : Δ$H_f$

Δ$H_f$ = ∑np Δ$H_f$ (products) – ∑np Δ$H_f$ (reactants)

Δ$H_f$ = [1(Δ$H_f$ $N_2$) + 4(Δ$H_f$ $H_2O$)] – [1(Δ$H_f$ $N_2O_4$) + 4(Δ$H_f$ $H_2$)]

Δ$H_f$ = [1(0) + 4(-241.8)] – [1(+9.16) + 4(0)]

Δ$H_f$  = [4(-241.8)] – [1(+9.16)] = 978.3 kJ

Learn more about Enthalpy here ;
brainly.com/question/16720480

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