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Suppose a 250. mL flask is filled with 0.50 mol of H20, 1.0 mol of Co2...
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 250. ml flask is filled with 0.50 mol of CO, 0.60 mol of NO and 2.0 mol of CO2. The following reaction becomes possible: NO2(g) + CO(g) = NO(g) + CO2(g) The equilibrium constant K for this reaction is 3.29 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. IM x 6 ?
Suppose a 500.mL flask is filled with 0.80 mol of CO, 0.90 mol of CO2 and 0.20mol of H2. The following reaction becomes possible: COg+H2Og--->CO2g+H2g The equilibrium constant K for this reaction is 6.70at the temperature of theflask.Calculate the equilibrium molarity of H2O. Round your answer to two decimal places.
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 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 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 250.mL flask is filled with 0.70mol of H2O, 0.60mol of CO2 and 1.9mol of H2. The following reaction becomes possible: +COgH2Og +CO2gH2g The equilibrium constant K for this reaction is 0.732 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
Suppose a 250 ml flask is filled with 1.0 mol of NO and 0.70 mol of NO . The following reaction becomes possible: NO3(8) + NO(g) - 2NO(8) The equilibrium constant K for this reaction is 5.78 at the temperature of the flask. Calculate the equilibrium molarity of NO3. Round your answer to two decimal places. Ом 3 ? Expiat tion Check 20:30 MCGHE AB
Suppose a 250 ml flask is filled with 0.30 mol of I, and 1.5 mol of HI. The following reaction becomes possible: H2(g) +12(g)=2HI(g) The equilibrium constant K for this reaction is 0.532 at the temperature of the flask. Calculate the equilibrium molarity of 12. Round your answer to two decimal places. Пм x s ?
Suppose a 250. ml flask is filled with 1.5 mol of Cl, and 1.3 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) 2HCl (8) The equilibrium constant K for this reaction is 0.560 at the temperature of the flask. Calculate the equilibrium molarity of H. Round your answer to two decimal places. OM * 5 ?