The equilibrium constant is 0.0900 at 25°C for the reaction H2O (g) + Cl2O (g) = 2HOCl(g) For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift? A 1.0-L flask contains 2.0 mole of HOCL, 0.20 mole of Cl2O, and 0.20 mole of H2O .   A 2.0-L flask contains 0.084 mole ofHOCl , 0.080 mole of Cl2O, and 0.98 mole of H2O  .   A 3.0-L flask contains 0.35 mole of HOCl , 0.0010 mole of Cl2, and 0.43 mole of H2O .

For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.220 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.

The equilibrium constant for the following reaction is 0.18 at a set temperature. Find the equilibrium concentrations if the initial concentration of PCl3 is 0.225 mol/L and the initial concentration of Cl2 is 0.150 mol/L. PCI3(g)+CI2(g)=PCI5(g)

The equilibrium constant, K, for the following reaction is 1.37×10-2 at 503 K. PCl5 (g)  PCl3 (g) +  Cl2 (g) An equilibrium mixture of the three gases in a 13.9 L container at 503 K contains 0.303 M PCl5,   6.44×10-2 M PCl3 and 6.44×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 6.07 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M

4 Titanium(IV) chloride decomposes to form titanium and chlorine, like this: Ticl,()-Ti(s)+2 Cl,(9) At a certain temperature, a chemist finds that a 7.7 L reaction vessel containing a mixture of titanium(IV) chloride, titanium, and chlorine at equilibrium has the following composition: compound amount TiCl, 4.90 g Ti 1.24 g Cl, 2.16 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K = 0 Submit Assignment Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility Finder F12 F11 F9 F10 F8 F7 F5 F6 .

The equilibrium constant, K, for the following reaction is 1.80×10-2 at 510 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 7.99 L container at 510 K contains 0.377 M PCl5,   8.23×10-2 M PCl3 and 8.23×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 18.5 L? [PCl5] =  M [PCl3] =  M [Cl2] =  M

An equilibrium mixture contains 0.700 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) ⇒ CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂ I mol

The equilibrium constant, K, for the following reaction is 5.10x10 at 548 K. NH4Cl(s) NH3(g) + HCI(g) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 548 K contains 0.368 mol NH4Cl, 2.26x10-3 M NH₂ and 2.26×10-³ M HCl. If the concentration of HCl(g) is suddenly increased to 3.22×103 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH₂] = [HCI] M M