consider-the-gaseous-equilibrium-for-the-dimerization-of-no2-no2-g-n2o4-g-what-i

Question

Consider the gaseous equilibrium for the dimerization of NO₂ at 350 K.

2 NO₂(g) ⇌ N₂O₄(g)

What is the value of ΔG when NO₂ = 1.23 atm and N₂O₄ = 2.45 atm? Use the following ΔG° values:

ΔG° (NO₂(g)) = 51.3 kJ/mol

ΔG° (N₂O₄(g)) = 99.8 kJ/mol

In which direction (forward or reverse) this reaction is spontaneous under the given conditions?

Accepted Answer

ΔG = −1.40 kJ
Since the value of ΔG is negative, the reaction is spontaneous in the forward direction.

Answer

ΔG = 3.15 kJ
Since the value of ΔG is positive, the reaction is spontaneous in the reverse direction.

Answer

ΔG = 1.95 kJ
Since the value of ΔG is positive, the reaction is spontaneous in the reverse direction.

Answer

ΔG = −2.85 kJ
Since the value of ΔG is negative, the reaction is spontaneous in the forward direction.