A 0.720-mole sample of PCI was placed into a 1.00 Liter container and heated to 300°C. At equilibrium the vessel contained 0.400 mol of PCI , along with Chlorine gas and unreacted PCI, What is the equilibrium constant for the decomposition of PCl at this temperature? (Hint writes the equation and figure out the equilibrium concentration of all species first.)

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The equilibrium constant, K for the following reaction is 4.43x10-2 at 638 K. An equilibrium mixture of the three gases in an 18.3 L container at 638 K contains 0.198 M COCI2, 9.37x10-2 M CO and 9.37x10-2 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 8.02 L? Be sure to report appropriate sig figs and units. COCI₂(g) CO(g) + Cl₂(g) [COC2] = [CO] = [Cl₂] = 4 N

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 25.0 L tank with 1.5 mol of ammonia gas and 2.4 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.60 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K_ = ] |x10 ?

Suppose a 250. mL flask is filled with 0.20 mol of Cl,, 1.0 mol of CHCI, and 2.0 mol of CCI,. The following reaction becomes possible: Cl, (g) +CHCI, (g) HC1(g)+CCl,(g) The equilibrium constant K for this reaction is 8.66 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. IM

An equilibrium mixture of PCI, (g), PCl, (g), and ClL, (g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl, (g) is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of mixing. The system then re-equilibrates. The chemical equation for this reaction is PCI, (g) + Cl, (g) PCl,(g) Calculate the new partial pressures, P, after equilibrium is reestablished. Torr Ppcl, Torr Pcı, Torr PPCI, II

At a certain temperature, 0.940 mol SO, is placed in a 2.00 L container. 2 SO, (g) = 2 SO,(g) + 0,(g) At equilibrium, 0.130 mol O, is present. Calculate K. K. =

Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 2.0 L flask with 2.3 atm of ammonia gas and 0.52 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of nitrogen gas to be 0.24 atm. Calculate the pressure equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits.

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 125. L tank with 11. mol of sulfur dioxide gas and 35. mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 7.7 mol. Calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K. = |

The molecule borneal can rearrange to a different form called isoborneal in a process called isomerization. A container initially contains only borneal gas at a pressure of 553 torr. At equilibrium, the pressure of borneall is 500.0 torr and the pressure of isoborneol is 53.0 torr. Is the isomerization reaction exergonic or endergonic? Calculate the value of the equilibrium constant for the reaction, borneal ⇌ isoborneol.