N2(g) + 3H2(g) ⇌ 2NH3(g)
ΔH° = −92 kJ
ΔS° = −0.20 kJ/K
Which of the given is correct about the ΔG° at 35 °C?
A. 30 kj
B. -62 kj
C. 62 kj
D. -30 kj
dG = dH - TdS but I'm confused about the problem. The dGo, by definition, is dG at 25C and not 35. You can calculate dG at 35 but then it isn't dGo.
To determine the correct option for ΔG° at 35 °C, we can use the equation:
ΔG° = ΔH° - TΔS°
Where:
ΔH° is the standard enthalpy change
ΔS° is the standard entropy change
T is the temperature in Kelvin
Let's calculate the value using the given equation:
ΔG° = -92 kJ - (35+273) K * (-0.20 kJ/K)
ΔG° = -92 kJ + 308 K * 0.20 kJ/K
ΔG° = -92 kJ + 61.6 kJ
ΔG° = -30.4 kJ
Therefore, the correct option for ΔG° at 35 °C is D. -30 kJ.