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.

Suppose a 500.mL flask is filled with 0.20mol of Cl2, 1.8mol of CHCl3 and 1.6mol of CCl4. The following reaction becomes possible:+Cl2gCHCl3g +HClgCCl4gThe equilibrium constant K for this reaction is 8.66 at the temperature of the flask.Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.

A 2.00 litre flask is filled with 1.5 mole SO3, 2.5 mole SO2, and 0.5 mole O2, and allowed to reach equilibrium. At this temperature, K = 1.0. Predict the effect on the concentration of O2 as equilibrium is being achieved by using Q, the reaction quotient.

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

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?