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.

Suppose a 250.mL flask is filled with 0.80mol of N2 and 1.1mol of O2. The following reaction becomes possible:+N2gO2g 2NOgThe equilibrium constant K for this reaction is 2.70 at the temperature of the flask.Calculate the equilibrium molarity of N2. Round your answer to two decimal places.M

For the reaction system: 2SO2(g) + O2(g)  ⇋   2SO3(g)the equilibrium concentrations are: [SO3] = 0.150 M; [SO2] = 0.940M; [O2] = 0.430MCalculate the value of K for the reactionQuestion 5Select one:a.16.9b.0.16c.2.7d.0.0590e.0.37

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?

One mole each of 2NO (g) and 2 4N O (g)were mixed in a 1 3dm flask and allowed toequilibrate. The following equilibrium wasestablished : 32 2 42NO (g) N O (g)If at equilibrium the reaction mixturecontained 0.75 moles of 2 4N O (g) , calculatethe value of equilibrium constant ck for thereaction

The equilibrium constant, KC, for the following reaction is 280 at 1,000 K.2SO2(g) + O2(g) ⇌ 2SO3(g)If [SO2]eq = 0.80 M and [O2]eq = 0.35 M, then [SO3]eq =