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Suppose a 500. mL flask is filled with 0.50 mol of H, and 1.7 mol of...
Suppose a 500 ml flask is filled with 0.50 mol of CO, 1.7 mol of H,0 and 1.1 mol of H. The following reaction becomes possible: CO(g) +H,0(8) -CO2() +H,() The equilibrium constant K for this reaction is 0.244 at the temperature of the flask. Calculate the equilibrium molarity of 1,0. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 0.50 mol of H2 and 1.9 mol of HI. The following reaction becomes possible: H2(g)+12g2HIg The equilibrium constant K for this reaction is 4.94 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places.
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 ?
Suppose a 500 mL. flask is filled with 1.9 mol of H, and 0 90 mol of HI. The following reaction becomes possible: H(8)+128)2HI) The equilibrium constant K for this reaction is 0.752 at the temperature of the flask. Calculate the equilibrium molarity of HI. Round your answer to two decimal places.
Suppose a 500. ml flask is filled with 1.7 mol of Cl, and 2.0 mol of HCl. The following reaction becomes possible: H2(g) +C12(g) + 2HCl (8) The equilibrium constant K for this reaction is 7.05 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. x o ?
Suppose a 250. ml flask is filled with 1.7 mol of H, and 0.30 mol of Cly. The following reaction becomes possible: H2(g) + Cl2(g) - 2HCI(g) The equilibrium constant K for this reaction is 6.15 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places. OM xo?
Suppose a 500. mL flask is filled with 1.5 mol of CO, 1.8 mol of H,O and 0.60 mol of CO,. The following reaction becomes possible: CO(g) +H2O(g) + CO2(g)+H2(g) The equilibrium constant K for this reaction is 3.75 at the temperature of the flask. Calculate the equilibrium molarity of 1,0. Round your answer to two decimal places. IM | xs ?
Suppose a 250. ml flask is filled with 0.10 mol of H and 0.30 mol of I. The following reaction becomes possible: H2(g) +12(g) - 2HI(g) The equilibrium constant K for this reaction is 5.61 at the temperature of the flask. Calculate the equilibrium molarity of H. Round your answer to two decimal places. OM x ?
Suppose a 250. ml flask is filled with 0.50 mol of H, and 0.40 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) = 2HCl (g) The equilibrium constant K for this reaction is 5.61 at the temperature of the flask. Calculate the equilibrium molarity of Cl. Round your answer to two decimal places. TOM xo?
Suppose a 500. mL flask is filled with 2.0 mol of I_2 and 0.40 mol of HI. The following reaction becomes possible: H_2(g) + IK_2(g) 2HI(g) The equilibrium constant K for this reaction is 9.22 at the temperature of the flask. Calculate the equilibrium molarity if I_2.