Phosphorous pentachloride decomposes according to the reaction PCI, (g) = PCI,(g) + Cl,(g) A 10.1 g sample of PCl, is added to a sealed 1.25 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 31.6% of the PCl, remains. What is the equilibrium constant, Ke , for the reaction?

Steam reforming of methane ( CH₁ ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 2.0 L flask with 2.6 atm of methane gas and 2.3 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 1.4 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K = Р x10 X Ś

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 200. mL flask with 3.5 atm of ammonia gas and 2.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of nitrogen gas to be 0.18 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 500. mL flask with 1.3 atm of sulfur dioxide gas and 2.5 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 0.39 atm. Calculate the pressure 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 P -D x10 X G

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -2 N,(g) + 3 H,(g) F2 NH,(g) K,=4. × 10 He fills a reaction vessel at this temperature with 9.0 atm of nitrogen gas and 4.5 atm of hydrogen gas. Use this data to answer the questions in the table below. O yes Can you predict the equilibrium pressure of NH, using only the tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of NH, at right. O. atm Round your answer to 1 significant digit. Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use I Privacy I Accessibility

Steam reforming of methane ( CHA) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 75.0 L tank with 34. mol of methane gas and 14. mol of water vapor, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 4.2 mol. Calculate the concentration equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K.- Explanation Check 2021 McGraw H E MacBook Air F10 F7 esc F3 F2 * # 2$ & @ 7 8

Suppose a 500. mL flask is filled with 1.7 mol of Br,, 1.4 mol of OCl, and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g)- BROC1(g)+BrC1(g) The equilibrium constant K for this reaction is 0.645 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. olo ? Ar G Explanation Check © 2022 McGraw Hill LLC. AIL Rights Reserved. Terms of Use | Privacy Center | Accessibility

At a particular temperature 8.0 mol NO2 gas is placed in a 1.0-L container. Over time the NO2 decomposes to NO and O2: 2NO2(g) 2 2NO(g) + O2(g) At equilibrium the concentration of NO(g) was found to be 1.8 mol/L. Calculate the value of K for this reaction (using units of mol/L for the concentrations). K =

Consider the reaction: 2 CO(g) + O₂(g) 2 CO₂(g). The reaction is allowed to reach equilibrium in a sealed vessel. According to Le Chatelier's principle, what will happen to the equilibrium, if the volume of the vessel is decreased while the temperature is kept constant? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will be unchanged, but the reaction will shift to the right. (D) The equilibrium constant will increase and the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.

Suppose a 250. mL flask is filled with 1.0 mol of Br2, 0.40 mol of OC12 and 1.7 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOCI (g) + BrC1 (g) The equilibrium constant K for this reaction is 0.681 at the temperature of the flask. Calculate the equilibrium molarity of OC12. Round your answer to two decimal places. M X