Suppose a 500.mL flask is filled with 0.30mol of Cl2, 0.40mol of CHCl3 and 1.5mol of CCl4. The following reaction becomes possible:+Cl2gCHCl3g +HClgCCl4gThe equilibrium constant K for this reaction is 8.88 at the temperature of the flask.Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.

Suppose a 500.mL flask is filled with 0.50mol of CO, 0.30mol of NO and 2.0mol of CO2. The following reaction becomes possible:+NO2gCOg +NOgCO2gThe equilibrium constant K for this reaction is 0.174 at the temperature of the flask.Calculate the equilibrium molarity of NO. Round your answer to two decimal places.M

Suppose a 500.mL flask is filled with 1.2mol of H2 and 2.0mol of HI. The following reaction becomes possible:+H2gI2g 2HIgThe equilibrium constant K for this reaction is 2.01 at the temperature of the flask.Calculate the equilibrium molarity of H2. Round your answer to two decimal places.

Methane and oxygen react to form water and carbon dioxide, like this:CH4(g)+2O2(g)→2H2O(g)+CO2(g)Use this chemical equation to answer the questions in the table below.Suppose 165.mmol of CH4 and 330.mmol of O2 are added to an empty flask. How much CH4 will be in the flask at equilibrium? None.Some, but less than 165.mmol.165.mmol.More than 165.mmol.Suppose 70.0mmol of H2O and 35.0mmol of CO2 are added to an empty flask. How much CH4 will be in the flask at equilibrium?

OCl2(g) ⇄ CO(g) + Cl2(g)COCl2(g) decomposes according to the equation above. When pure COCl2(g) is injected into a rigid, previouslyevacuated flask at 690 K, the pressure in the flask is initially 1.0 atm. After the reaction reaches equilibrium at 690K, the total pressure in the flask is 1.2 atm. What is the value of Kp for the reaction at 690 K

or the equilibriumPCl5(g) → PCl3 (g) + Cl2 (g)Kc = 0.19 mol dm-3 at 250°CThe equilibrium mixture at this temperature contains PCl5 at a concentration of 0.20 moldm-3 and PCl3 at a concentration of 0.010 mol dm-3 . Calculate the concentration of Cl2 inthis mixture