= Objective Knowledge Check Question 12 Suppose a 250 ml flask is filled with 1.6 mol...
Suppose a 500 ml flask is filled with 0.10 mol of Bry, 1.6 mol of OCI, and 0.60 mol of BrCl. The following reaction becomes possible: Bry()+OCI (8) -BrOCI () + BrCl() The equilibrium constant K for this reaction is 0.770 at the temperature of the flask Calculate the equilibrium molarity of OCI. Round your answer to two decimal places x x 5 ?
Suppose a 250. mL flask is filled with 1.0 mol of Br,, 1.5 mol of OCI, and 1.8 mol of BrOCI, The following reaction becomes possible: Br (8)+OCI,(8)BroCI (e) + BrCl(e) The equilibrium constant K for this reaction is 0.913 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places.
Suppose a 250. ml flask is filled with 1.8 mol of OC1, 0.70 mol of BroCl and 0.50 mol of BrCl. The following reaction becomes possible: Br2(g) + OC12(g) – Brocl(g) +BrCl(g) The equilibrium constant K for this reaction is 1.48 at the temperature of the flask. Calculate the equilibrium molarity of BroCl. Round your answer to two decimal places. x 5 ?
Objective Knowledge Check Suppose a 250. mL flask is filled with 0.20 mol of H20, 0.10 mol of CO2 and 1.5 mol of Hy. The following reaction becomes possible: COG) + H2O@eCO3%)+H,®) The equilibrium constant for this reaction is 4.23 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places Ом $ ?
Suppose a 500. mL flask is filled with 0.90 mol of OC1,, 0.20 mol of BroCl and 1.4 mol of BrCl. The following reaction becomes possible: Br2(g) +OC12(g) =BroCl(g) +BrCl(g) The equilibrium constant K for this reaction is 0.798 at the temperature of the flask. Calculate the equilibrium molarity of Br2. Round your answer to two decimal places. IM xs ?
Suppose a 500. ml flask is filled with 1.3 mol of Br2, 2.0 mol of OC1, and 1.2 mol of BrCl. The following reaction becomes possible: Br2(g) + OC12(g) = BroCl (g) + BrCl (g) The equilibrium constant K for this reaction is 0.766 at the temperature of the flask. Calculate the equilibrium molarity of OC12. Round your answer to two decimal places. xs ?
Objective Knowledge Check Suppose a 250. mL flask is filled with 0.20 mol of H,O, 0.10 mol of CO, and 1.5 mol of H,. The following reaction becomes possible: (H+)00(3oH+)0 The equilibrium constant K for this reaction is 4.23 at the temperature of the flask Calculate the equilibrlum molarity of CO. Round your answer to two decimal places. M ?
Suppose a 250. mL flask is filled with 2.0 mol of Br2, 1.1 mol of OCI, and 0.80 mol of BroCl. The following reaction becomes possible: Br2(g) + Oci (g) Broci (g) + Brci(g) The equilibrium constant K for this reaction is 0.624 at the temperature of the flask. Calculate the equilibrium molarity of BroCl. Round your answer to two decimal places. Пм xs ?
Suppose a 250. ml flask is filled with 1.6 mol of Cl, and 1.3 mol of HCI. The following reaction becomes possible: H2(g) + Cl2(g) → 2HCI (g) The equilibrium constant K for this reaction is 0.967 at the temperature of the flask. Calculate the equilibrium molarity of C1. Round your answer to two decimal places. OM I ?
Suppose a 500 ml flask is filled with 1.6 mol of H, and 1.7 mol of HCl. The following reaction becomes possible: H2(g) +C12(g) + 2HCI(g) The equilibrium constant K for this reaction is 8.78 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. OM x 6 ?