An equilibrium mixture contains 0.870 M H2O, 0.870 M Cl2O, and 0.261 M HOCl. How many moles of Cl2O would need to be added at constant temperature and volume to increase the final concentration of HOCl to 0.356 M once equilibrium is reestablished in a 1.00 L container

Steam reforming of methane (CH) 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 125. L tank with 34. mol of methane gas and 11. mol of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be 7.7 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 = 0 X

Suppose a 250. mL flask is filled with 1.2 mol of Br₂, 0.50 mol of BrOCl and 1.9 mol of BrC1. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrC1 (g) The equilibrium constant K for this reaction is 0.156 at the temperature of the flask. Calculate the equilibrium molarity of OC12. Round your answer to two decimal places. |] M X Ś ?

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

Initially, 0.1500 mol of SO3(g) were placed in a 1.00 L reaction vessel, heated to a high temperature and allowed to come to equilibrium according to the reaction 2 SO3(g) → 2 SO₂(g) + O2(g) Kc = ? It was found that the equilibrium concentration of SO₂(g) was 0.1424 M. What is the equilibrium constant, Kc, for the reaction at this temperature? A. 0.041 ✓B. 25 C. 0.064 D. 98

Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2 (g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.300 mol N2 and 0.980 mol O2 are mixed in a 5.00-L reaction vessel. What will be the concentrations of N2, O2, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small—less than 10% of the starting amounts—and check your assumption when you have solved the equation.)

Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. 1.80 at 250 °C A 0.2950 mol sample of PCl, (g) is injected into an empty 4.75 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCl,] = M [PCI,] = M

Steam reforming of methane ( CH ) 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 25.0 L tank with 7.0 mol of methane gas and 1.8 mol of water vapor, and when the mixture has come to equilibrium measures the amount of carbon monoxide gas to be 1.4 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 = || %3D Submit Assignn

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 5.0 L flask with 4.3 atm of sulfur dioxide gas and 3.9 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 3.9 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, = 0

Given 0.50 mol of NOCI is placed in a one-liter reaction vessel at 700 K and after the system comes to equilibrium the concentration of NOCI became 0.440 M. What is the equilibrium constant? Given the reaction as: 2NOCI(g) → 2NO(g) +Cl2(g) 5.6 x 10-4 2.0 x 10-3 4.1 x 10-3 6.1 x 10-3 8.2 x 10-3