Consider the following equilibrium system involving SO2, Cl2, and SO2Cl2 (sulfuryl dichloride): SO2(g) + Cl2(g)  ⇌ SO2Cl2(g) Predict how the equilibrium position would change if the temperature remains constant and if Cl2 gas was added to the system.  SO2Cl2 was removed from the system. SO2 was removed from the system.

Consider the following equilibrium system at 355 K. 2NOBr(g) -----> 2NO(g)+Br2(g). If an equilibrium mixture of the three gases at 355 K contains 3.21x10^-2 M NOBr, 2.01x10^-2 M NO,and 3.98x10^-2 M Br2 what is the value of the equilibrium constant K

For the following reaction, the equilibrium constant Keq is 6.40 x 10-7 at 2000°C. 2CO2 (g)  2CO (g) + O2 (g) If 0.250 moles of CO2(g) is introduced into a 1.00 L vessel, calculate the equilibrium concentrations of CO(g) and O2(g) at this temperature.

Sulfur dioxide and oxygen react to form sulfur trioxide, like this: 2 SO,(9) + 0,(9) → 2 SO3(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of sulfur dioxide, oxygen, and sulfur trioxide has the following composition: compound concentration at equilibrium SO2 0.78M O, 1.5M SO3 0.94M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits.

Calculate the equilibrium concentrations for all reactants and products if initial concentrations of CH4 is 0.400 M, H2S is 0.800 M, CS2 is 0.400 M, H2 is 0.800 M are mixed and allowed to establish equilibrium.  The Kc for the reaction is 0.0360 and the equilibrium concentration of CH4is 0.556 M.   CH4(g) + 2H2S(g) ↔  CS2(g) + 4H2(g) Group of answer choices [CH4] = 0.556 M, [H2S] = 0.488 M, [CS2] = 0.556 M, [H2] = 1.42 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.244 M, [H2] = 0.176 M. [CH4] = 0.556 M, [H2S] = 0.244 M, [CS2] = 0.956 M, [H2] = 1.36 M. [CH4] = 0.556 M, [H2S] = 1.11 M, [CS2] = 0.556 M, [H2] = 1.42 M.

The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g)If an equilibrium mixture of the three compounds in a 6.01 L container at 298 K contains 4.00 mol of NH4HS(s) and 0.432 mol of NH3, the number of moles of H2S present is moles.

Equilibrium constant, Kc, for the following reaction is 8.08×10-3 at 1080 K.2SO3(g) 2SO2(g) + O2(g)Calculate the concentration of SO3 in the equilibrium mixture?When a sufficiently large sample of SO3(g) is introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2(g) is found to be 9.70×10-2 M.

Consider the equilibrium reaction:2 SO2 (g) + O2(g) ⇌ 2SO3(g)In a particular experiment a student added 0.0870 moles of SO2 and 0.0780 moles of O2 to a 0.750-L container. At equilibrium, the equilibrium concentration of O2 was 0.065 molar. What is the value of the equilibrium constant K?

Calcium oxide and carbon dioxide react to form calcium carbonate, like this: CaO(s)+CO2(g)→CaCO3(s) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of calcium oxide, carbon dioxide, and calcium carbonate at equilibrium has the following composition: compound amount Cao 31.2 g CO2 16.8 g CACO3 32.3 g Calculate the value of the equilibrium constant K̟ for this reaction. Round your answer to 2 significant digits. K = [| Submit A Continue MacBook Air F10

Mercury and oxygen react to form mercury(II) oxide, like this: 2 Hg(1)+O2(g)→2 HgO(5) At a certain temperature, a chemist finds that a 3.6 L reaction vessel containing a mixture of mercury, oxygen, and mercury(II) oxide at equilibrium has the following composition: compound amount Hg 9.7 g O2 21.8 g HgO 10.2 g Calculate the value of the equilibrium constant K̟ for this reaction. Round your answer to 2 significant digits. K_ = 0