Dinitrogen tetroxide decomposes according to
N₂O₄(g) ⇌ 2 NO₂(g)
At 298 K the standard free-energy change for the forward reaction is ΔG° = +4.8 kJ·mol⁻¹. A sealed flask at 298 K contains 0.10 atm N₂O₄ and 1.0 atm NO₂. What is the value of ΔG (in kJ·mol⁻¹) for the reaction under these conditions?
(R = 8.314 J·mol⁻¹·K⁻¹)
a) −1.0kJ mol−1
b) +10.5kJ mol−1
c) +5.7kJ mol−1
d) +7.3kJ mol−1