The equilibrium constant for the following reaction is 3.5 × 10⁸ at 25°C. N₂ (g) + 3H₂ (g) 2NH₃ (g)
The value of ΔG° for this reaction is __________ kJ/mol.

Question

The equilibrium constant for the following reaction is 3.5 × 10⁸ at 25°C. N₂ (g)+ 3H₂ (g) 2NH₃ (g) The value of ΔG° for this reaction is __________ kJ/mol.

Quizplus · Accepted Answer

The formula relating ΔG° to the equilibrium constant is:
ΔG° = -RTlnK
where R is the gas constant (8.314 J/mol·K), T is the temperature in Kelvin (25°C = 298 K), and K is the equilibrium constant.
Plugging in the values:
ΔG° = -(8.314 J/mol·K)(298 K)ln(3.5×10^18)
ΔG° = -49.1 kJ/mol (rounded to one decimal place)
Therefore, the correct answer is D (-49).

The Equilibrium Constant for the Following Reaction Is 3