Question

The equilibrium constant for the following reaction is 9.13 at 740 k. 2nh3(g) = n2(g) 3H₂(g). Calculate kc at this temperature for the following reaction: nh3(g) = 1/2n2(g) 3/2H₂(g)

Answer 1

The equilibrium constant Kc for the reaction NH3(g) => 1/2 N2(g) + 3/2 H2(g) is the square root of the Kc for the reaction 2 NH3(g) => N2(g) + 3 H2(g), which is approximately 3.02 at 745 K.

Step-by-step explanation:

The subject of the question is Chemistry, specifically related to the calculation of equilibrium constants at a given temperature. The equilibrium constant Kc for the first given reaction 2 NH3(g) => N2(g) + 3 H2(g) at 745 K is 9.13. To find the Kc for the second reaction NH3(g) => 1/2 N2(g) + 3/2 H2(g), we must understand that the relationships between equilibrium constants of related chemical reactions are determined by stoichiometry. If we take the square root of the equilibrium constant for the reaction 2 NH3(g) => N2(g) + 3 H2(g), which has a Kc of 9.13, we can find the Kc for the half-reaction NH3(g) => 1/2 N2(g) + 3/2 H2(g), since the stoichiometric coefficients in the second reaction are exactly half of those in the first reaction. The square root of 9.13 is approximately 3.02, so the Kc for the second reaction is 3.02 at 745 K.