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 0.70mol of H2O, 0.60mol of CO2 and 1.9mol of...
Suppose a 250.mL flask is filled with 0.90mol of CO , 1.8mol of H2O and 1.5mol of H2 . The following reaction becomes possible: +COgH2Og +CO2gH2g The equilibrium constant K for this reaction is 0.930 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 0.50 mol of H20, 1.0 mol of Co2 and 1.5 mol of H2. The following reaction becomes possible cog)+H20(g)Co()+H28) The equilibrium constant K for this reaction is 4.10 at the temperature of the flask Calculate the equilibrium molarity of H20. Round your answer to two decimal places.
Suppose a 250.mL flask is filled with 1.0mol of NO2 , 0.40mol of CO and 0.10mol of CO2 . The following reaction becomes possible: +NO2gCOg +NOgCO2g The equilibrium constant K for this reaction is 7.16 at the temperature of the flask. Calculate the equilibrium molarity of NO2 . Round your answer to two decimal places.
Costa Suppose a 250 ml flask is filled with 1.4 mol of CO, 2.0 mol of H,0 and 0.10 mol of CO2. The following reaction becomes possible: CO(g)+H2O(g) + CO2(g)+H,(g) The equilibrium constant K for this reaction is 0.504 at the temperature of the flask. Calculate the equilibrium molarity of CO,. Round your answer to two decimal places. Ом X 5 ?
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 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 250.mL flask is filled with 1.9mol of H2 and 1.7mol of I2. The following reaction becomes possible: H2(g) + I2(g) 2HI(g) The equilibrium constant K for this reaction is 5.99 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 0.30 mol of H2 and 1.3 mol of HI. The following reaction becomes possible: H2(8)+12)2HIg) The equilibrium constant K for this reaction is 0.254 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places. Ar
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 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 ?