This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Write the equilibrium constant expression (K_c) for the reaction. The given reaction is: N_2(g) + 3H_2(g) 2NH_3(g) The equilibrium constant expression for this reaction is: K_c = [NH_3]^2[N_2][H_2]^3 Step 2: Substitute the given equilibrium concentrations into the expression. The given equilibrium concentrations are: [N_2] = 0.5 mol/litre [H_2] = 0.5 mol/litre [NH_3] = 0.15 mol/litre Substitute these values into the K_c expression: K_c = (0.15 mol/litre)^2(0.5 mol/litre)(0.5 mol/litre)^3 Step 3: Calculate the value of K_c. K_c = 0.0225 (mol/litre)^2(0.5 mol/litre)(0.125 (mol/litre)^3) K_c = 0.0225 (mol/litre)^20.0625 (mol/litre)^4 K_c = 0.36 (mol/litre)^-2 K_c = 0.36 L^2/mol^2 The value of K_c is 0.36 L^2/mol^2.