![H2(g) + I2(g) <=> 2HI(g) [ H2] = 0.50 mol/dm3 [ I2] = 0.20 mol/dm3 [* HI] = 1.00 mol/dm3 Calculate Kc](/_next/image?url=https%3A%2F%2Fohijasnjvprzodcmxltt.supabase.co%2Fstorage%2Fv1%2Fobject%2Fpublic%2Fwhatsapp-images%2F1784154923884-ff82bfecdd340865.png&w=3840&q=75)
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 for the given reaction. The balanced chemical equation is: H_2(g) + I_2(g) 2HI(g) The equilibrium constant K_c is expressed as the ratio of the product concentrations raised to their stoichiometric coefficients to the reactant concentrations raised to their stoichiometric coefficients. K_c = [HI]^2[H_2][I_2] Step 2: Substitute the given equilibrium concentrations into the K_c expression. Given concentrations at equilibrium are: [H_2] = 0.50 mol/dm^3 [I_2] = 0.20 mol/dm^3 [HI] = 1.00 mol/dm^3 K_c = (1.00 mol/dm^3)^2(0.50 mol/dm^3)(0.20 mol/dm^3) Step 3: Calculate the value of K_c. K_c = 1.00 (mol/dm^3)^20.10 (mol/dm^3)^2 K_c = 10.0 The value of K_c is 10.0. That's 2 down. 3 left today — send the next one.