Methanol and oxygen react to form carbon dioxide and water, like this: 2 CH;OH(1)+3 O,(9)→2CO,(9)+4H,O(g) At a certain temperature, a chemist finds that a 2.6 L reaction vessel containing a mixture of methanol, oxygen, carbon dioxide, and water at equilibrium the following composition: compound amount CH,OH 1.64 g 1.70g co, 2.46 g H,O 247g Calculate the value of the equilibrium constant K. for this reaction. Round your answer to 2 significant digits.

Suppose a 250. mL flask is filled with 1.2 mol of OCl,, 1.9 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br,(g) +OCl,(g) BROCI(g) +BrC1(g) The equilibrium constant K for this reaction is 1.94 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.

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 .

A gaseous mixture contains 0.27 mol CO, 0.12 mol H2, and 0.022 mol H,O, plus an unknown amount of CH4, in each liter. This mixture is at equilibrium at a certain temperature. CO(9) + 3H, (9) = CH4 (9) + H,O(9) What is the concentration of CH4 in this mixture? The equilibrium constant K, equals 3.99.

Coal can be used to generate hydrogen gas (a potential fuel) by the following endothemic reaction (heat is on the reactant side of the equation). C (3) + H20 (g) = co (g) + H2 (g) If this reaction mixture is at equilibrium, predict whether each of the following will resuit in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. Part A adding more C to the reaction mixture the formation of additional hydrogen gas the formation of less hydrogen gas O no effect on the quantity of hydrogen gas

O KINETICS AND EQUILIBRIUM Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 380.: NO,(8) + CO(3) = NO(g) + CO,(3) Use this information to complete the following table. Suppose a 16. L reaction vessel is filled with 1.4 mol of NO, and 1.4 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little No, and CO. O There will be very little NO and CO,. O Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] NO(9)+CO,(9) NO,(9)+CO(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = ] %3D 3 NO,(9)+3CO(g) 3 NO(g)+3CO,(9) 1L Explanation Check III

Consider the following equilibrium   If the equilibrium concentration of chlorine and phosphorous trichloride are 0.80 mol/L and 0.70 mol/L, respectively,find the equilibrium concentration of phosphorous pentachloride.

Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s) + 3 H₂O(g) → Fe₂O3(s)+ 3 H₂(g) At a certain temperature, a chemist finds that a 2.5 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound Fe H₂O Fe₂O3 H₂ amount 4.04 g 2.87 g 3.49 g 2.08 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. C K = 0 C Dx1 x10 X Ś

Consider the following reaction: 2NH3(g) N₂(g) + 3H₂(g) If 5.40x10-4 moles of NH3(g), 0.450 moles of N₂, and 0.215 moles of H₂ are at equilibrium in a 15.1 L container at 846 K, the value of the equilibrium constant, K, is

Calculating an equilibrium constant from a partial equilibrium composition 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 1.2 atm of ammonia gas and 3.7 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of water vapor to be 1.3 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. K = [] P x10 X ? olo 18 Ar 8.