## N2 (g) + 3 H2 (g) → 2 NH3 (g)

Back to reactions list

Synthesis

## Stoichiometry

Enter a mass or volume in one of the boxes below. Upon hitting submit, the stoichiometric equivalents will be calculated for the remaining reactants and products. All gases are assumed to be at STP.

 N2             Mass: g or Gas Volume: L H2             Mass: g or Gas Volume: L NH3            Mass: g or Gas Volume: L Heat Released: kJ

## Enthalpy of Reaction

[2ΔHf(NH3 (g))] - [1ΔHf(N2 (g)) + 3ΔHf(H2 (g))]
[2(-46.11)] - [1(0) + 3(0)] = -92.22 kJ
-92.22 kJ     (exothermic)

## Entropy Change

[2ΔSf(NH3 (g))] - [1ΔSf(N2 (g)) + 3ΔSf(H2 (g))]
[2(192.34)] - [1(191.5) + 3(130.59)] = -198.59 J/K
-198.59 J/K     (decrease in entropy)

## Free Energy of Reaction (at 298.15 K)

From ΔGf° values:
[2ΔGf(NH3 (g))] - [1ΔGf(N2 (g)) + 3ΔGf(H2 (g))]
[2(-16.48)] - [1(0) + 3(0)] = -32.96 kJ
-32.96 kJ     (spontaneous)

From ΔG = ΔH - TΔS:
-33.01 kJ     (spontaneous)

## Equilibrium Constant, K (at 298.15 K)

595200.76026
This process is favorable at 25°C.

## Reference(s):

Ebbing, Darrell D. General Chemistry 3rd ed.; Houghton Mifflin Company: Boston, MA, 1990; pp 115, 175, 223-4, 227.
Kotz, John C. and Treichel, Paul. Chemistry & Chemical Reactivity 4th ed.; Thomson Brooks/Cole: Belmont, CA, 1999; p 172.
Zumdahl, Steven and Zumdahl, Susan A. Chemistry 9th ed.; Brooks/Cole: Belmont, CA, 2014; p 132.