Answer:
To find the value of Kc for the given reaction at 400 K, use the relationship between Kp and Kc and stoichiometry to calculate the equilibrium constant. The correct value of Kc is 2.3 x 10⁻⁵.
The value of Kc for the reaction N₂(g) + 3 H₂(g) → 2 NH₃(g) at 400 K can be calculated using the relationship between Kp and Kc: To do this, we use the relationship $Kp = Kc(RT)^{(\Delta n)$ , where Δn is the change in moles of gas (products minus reactants), R is the ideal gas constant (0.0821 L·atm/(K·mol)), and T is the temperature in Kelvin.
Convert Kp to Kc using the equation $Kp = Kc(RT)^{(\Delta n)$ , where Δn = (moles of gaseous products) - (moles of gaseous reactants).
Plugging in the values given (Kp = 41) and the stoichiometry of the reaction (Δn = 2 - 1 - 3 = -2 for this reaction), you can calculate Kc to be 2.3 x 10⁻⁵.
Therefore, the answer is 3) 2.3 x 10⁻⁵.
